Chemistry Latex ~ Smart Edition Academy

What is the conjugate acid in the following equation?

CH₃COOH + H₂ O ⇌ H₃O^+ +CH₃COO^-

H₃O^+
H₂O
CH₃COO^-
CH₃COOH

Which would turn litmus paper blue?

HF
KOH
HNO₃
C₃H₆O₃

What happens to a Brnsted-Lowry base in an aqueous solution?

Donates hydrogen ions
Accepts a pair of electrons
Dissociates to hydronium ions
Increases hydroxide ion concentration

Which product completes the following acid-base reaction?

H₂ SO₄+2KOH → ?

H₃O⁺
HSO₃⁻
K₂SO₄
KHSO₄

What is the conjugate base of sulfuric acid?

HSO₄⁻
HSO₂⁻
HSO₃
H₂SO₃

What is formed when nitric acid (HNO₃) reacts with barium hydroxide (Ba(OH)₂)?

H₂O
HNO₂
Ba(NO₂)₂
Ba(NH₂)₂

Which of the following is an acid?

KNO₃
BaCl₂
NaOH
(H₃PO₄)

Which ions from a base react with hydrogen ions in a neutralization reaction?

CH₃⁺
(OH⁻)
H₃O⁺
COOH⁻

Using the following pH scale, which substance would be slippery to the touch when dissolved in water?

Borax
Coffee
Potato
Vinegar

What product is formed when acetic acid (CH₃COOH) reacts with water?

H₂
OH⁻
CH₃COO⁻
CH₃COOH₂

What conjugate base is produced when the Brnsted-Lowry acid hydrogen phosphate \((HPO_4^{2-})\) reacts with a hydroxide ion?

\(PO_3\)
\(H_2O\)
\(PO_4^{3-}\)
\(H_3O^+\)

Which is a characteristic of a basic solution?

Tastes sour
Accepts OH⁻ ions
Turns litmus blue
Contains a lot of H₃O⁺ ions

What is the conjugate base in the following reaction?

HNO₂+H₂O ↔ ?

OH⁻
NO₂⁻
H₃O⁺
HNO₃⁻

Using the following image, what substance is most likely a weak acid?

Antacid
Borax
Milk
Salmon

When HNO₃ reacts with NaOH, which product is formed?

OH⁻
H₃O⁺
NaH
NaNO₃

What is the conjugate acid of S²⁻?

HS⁻
H₂S
HS₃
HS²⁻

Which partially dissociates into hydroxide ions in an aqueous solution?

KOH
HClO₄
C₅H₅N
H₂CO₃

An acid that dissociates into hydrogen ions is defined as a(n)

weak acid.
Arrhenuis acid.
conjugate acid.
Br𝜙nsted-Lowry acid.

Which of the following is a strong acid?

HF
HCl
H₃PO₄
CH₃COOH

Which of the following would completely ionize in solution?

HF
HCl
N₂H₄
C₂H₄O₂

In which compound(s) does a chlorine atom share two electrons with another atom?

OCl₂ only
OCl₂ and Cl₂ only
SiCl₄, PCl₃, and OCl₂ only
SiCl₄, PCl₃, OCl₂, and Cl₂

Octane in gasoline has the formula C₈H₁₈.

What type of compound is it, and why?

Ionic, because it contains a metal
Covalent, because it contains a metal
Ionic, because it does not contain a metal
Covalent, because it does not contain a metal

In the molecule of chlorine (Cl₂) shown below, how is each chlorine atom stable?

Each chlorine atom shares one electron and has six lone-pair electrons.
Each chlorine atom shares six electrons and has one lone-pair electron.
Each chlorine atom shares two electrons and has six lone-pair electrons.
Each chlorine atom shares six electrons and has two lone-pair electrons.

In the compound silicon tetrachloride (SiCl₄) shown below, how is silicon stable?

Silicon shares a total of four electrons.
Silicon shares a total of eight electrons.
Silicon gives eight electrons to surrounding chlorine atoms.
Silicon removes four electrons from surrounding chlorine atoms.

In the Lewis structures below, which element is stable with four shared and four lone-pair electrons?

Chlorine
Oxygen
Phosphorus
Silicon

Consider the carbon-carbon bonds that exist in the molecules shown below.

Which of the compounds below contains the strongest carbon-carbon bond?

Acetylene
Ethane
Ethylene
Methanol

According to the Lewis structure below, what is the formula for methanol?

CHO
CH₃O
CH₄O
C₃HO

The compound silver sulfide has the formula Ag₂S.

Which of the following best describes the meaning of the subscript 2 in the formula?

The silver ion has a charge of -2.
The silver ion has a charge of +2.
There are two silver ions for every one sulfide ion.
There are two sulfide ions for every one silver ion.

In the compound sodium bromide (NaBr), electrons are _____.

In the compound carbon tetrabromide (CBr₄), electrons are _____.

shared, shared
shared, transferred
transferred, shared
transferred, transferred

What is the net charge of the ionic compound barium iodide (BaI₂)?

-1
0
1
2

In the Lewis structure of a fluorine molecule shown below, how are the eight valence electrons of each fluorine atom arranged?

2 are shared, 6 are lone-pair.
4 are shared, 4 are lone-pair.
6 are shared, 2 are lone-pair.
8 are shared, none are lone-pair.

Out of the elements present in the Lewis structures below, which one has the greatest number of shared electrons? Consider only single atoms of each element.

Chlorine
Oxygen
Phosphorus
Silicon

What is the formula for the compound formed between calcium and oxygen?

CaO
CaO₂
Ca₂O
Ca₃O₂

In the Lewis structure for carbon dioxide shown below, how many electrons is the carbon atom sharing with one oxygen atom?

2
4
5
6

In the dimensional analysis below, what is the unit of the final answer?

\(\frac{(2.25\times10^{24} atoms Pd)}{1}\times\frac{(1 mol Pd)}{(6.02\times10^{23} atoms Pd)}\times\frac{(106.42 g Pd)}{(1 mol Pd)}=398\) ?

atoms Pd
g Pd
g/mol Pd
mol Pd

A reaction requires 0.446 moles of calcium to produce a desired quantity of 25.0 grams of calcium oxide (CaO). What mass of calcium is required for this reaction?

1.60 g Ca
11.2 g Ca
17.9 g Ca
25.0 g Ca

In the dimensional analysis shown below, which unit(s) cancel out?

\(\frac{(42.5 g NH_3)}{1}\times\frac{(1 mol NH_3)}{(17.04 g NH_3 )}\times\frac{(6.02\times10^{23} molecules NH_3)}{(1 mol NH_3 )}=1.50\times10^{24} molecules NH_3\)

Grams of \(NH_3\)
Grams and moles of \(NH_3\)
Moles and molecules of \(NH_3\)
Grams, moles, and molecules of \(NH_3\)

A reaction requires \(8.41 \times 10^{23}\) molecules of phosphorus trichloride \((PCl_3)\). What mass of \((PCl_3)\) is needed?

0.102 g \(PCl_3\)
1.4 g \(PCl_3\)
98.3 g \(PCl_3\)
192 g \(PCl_3\)

Which statement is true about 1 mole of carbon monoxide (CO)? (Refer to the Periodic Table of Elements).

It contains \(2\) molecules.
It contains \(28.0\) molecules.
It has a mass of \(28.0\) grams.
It has a mass of \(6.02 \times 10^{23}\) grams.

A balloon at a birthday party contains 1.05 grams of helium. How many atoms of helium are in the balloon?

\(1.43 \times 10^{23}\) atoms He
\(1.50 \times 10^{23}\) atoms He
\(1.58 \times 10^{23}\) atoms He
\(2.53 \times 10^{24}\) atoms He

A roll of aluminum foil has a mass of 340. grams. How many moles are in the roll of aluminum?

\(12.6\) mol Al
\(9170\) mol Al
\(1.77 \times 10^{21}\) mol Al
\(2.05 \times 10^{26}\) mol Al

How many molecules are in 0.470 moles of silicon tetrachloride \((SiCl_4)\)?

\(79.9\) molecules \((SiCl_4)\)
\(361\) molecules \((SiCl_4)\)
\(2.83 \times 10^{24}\) molecules \((SiCl_4)\)
\(1.28 \times 10^{24}\) molecules \((SiCl_4)\)

How many moles of magnesium oxide (MgO) are in a sample containing \(4.36 \times 10^{23}\) particles?

\(0.724\) mol MgO
\(1.31\) mol MgO
\(1.08 \times 10^{23}\) mol MgO
\(1.76 \times 10^{25}\) mol MgO

One mole of iron is equal to _____.

\(1\) atom of iron
\(55.85\) grams of iron
\(55.85\) atoms of iron
\(6.02 \times 10^{23}\) grams of iron

What is the unit for the final answer in the dimensional analysis shown below?

\(\frac{(48.2 g FeCl_3)}{1}\times\frac{(1 mol FeCl_3)}{(162.20 g FeCl_3 )}\times\frac{(3 mol Cl_2)}{(2 mol FeCl_3 )}\times\frac{(70.9 g Cl_2)}{(1 mol Cl_2 )}=31.6 \)?

g \(Cl_2\)
g \(FeCl_3\)
mol \(Cl_2\)
mol \(FeCl_3\)

What is the molar mass of \(Fe(OH)_2\)?

72.86 g/mol
73.87 g/mol
89.87 g/mol
145.72 g/mol

Ethanol \((C_2H_5OH)\) is burned as fuel in the presence of oxygen to produce carbon dioxide \((CO_2)\) and water \((H_2O)\). According to the balanced chemical reaction shown below, two molecules of ethanol require _____ molecules of oxygen to react and produce _____ molecules of carbon dioxide and _____ molecules of water.

\(C_2H_5OH + 3O_2 \rightarrow 2CO_2 + 3H_2O\)

2, 2, 3
3, 2, 3
6, 2, 6
6, 4, 6

A reaction requires 0.35 moles of bromine \((Br_2)\). If bromine has a density of 3.1 g/mL, how many milliliters are required?

8.86 mL
18.0 mL
51.5 mL
173 mL

Propane gas \((C_3H_8)\) combusts according to the equation below. How many grams of carbon dioxide \((CO_2)\) are produced from 100. grams of propane?

\(C_3H_8 + 5O_2 \rightarrow 3CO_2 + 4H_2O\)

6.80 g \((CO_2)\)
99.8 g \((CO_2)\)
299 g \((CO_2)\)
1,470 g \((CO_2)\)

A can of cola contains 106 grams of sugar (\(C_{12}H_{22}O_{11}\)). Explain why it contains more or less than 1 mole of sugar.

Less than 1 mole because the molar mass is less than 106 g/mol.
More than 1 mole because the molar mass is less than 106 g/mol.
Less than 1 mole because the molar mass is greater than 106 g/mol.
More than 1 mole because the molar mass is greater than 106 g/mol.

Aluminum and chlorine react according to the reaction below. How many molecules of chlorine \((Cl_2)\) are required to form 28 grams of aluminum chloride \((AlCl_3)\)?

\(2Al + 3Cl_2 \rightarrow 2AlCl_3\)

\(2.2 \times 10^{22}\) molecules \((Cl_2)\)
\(1.3 \times 10^{23}\) molecules \((Cl_2)\)
\(1.9 \times 10^{23}\) molecules \((Cl_2)\)
\(2.5 \times 10^{25}\) molecules \((Cl_2)\)

Aluminum and chlorine react according to the reaction below. How many molecules of chlorine \((Cl_2)\) are required to form 28 grams of aluminum chloride \((AlCl_3)\)?

\(2Al + 3Cl_2 \rightarrow 2AlCl_3\)

\(2.2 \times 10^{22}\) molecules \((Cl_2)\)
\(1.3 \times 10^{23}\) molecules \((Cl_2)\)
\(1.9 \times 10^{23}\) molecules \((Cl_2)\)
\(2.5 \times 10^{25}\) molecules \((Cl_2)\)

In the chemical equation below, which element(s) are unbalanced?

\(Ba(C_2H_3O_2)_2 + Na_2SO_4 \rightarrow NaC_2H_3O_2 + BaSO_4\)

Sodium only
Barium and sodium
Carbon, hydrogen, and oxygen
Sodium, carbon, hydrogen, and oxygen

Which of the following conversion factors will be used to complete the dimensional analysis, given the balanced equation below?

\(Mg + 2HCl \rightarrow MgCl_2 + H_2\)

\(\frac{0.75 mol \hspace{0.2mm}HCl}{1}\times\frac{( ? )}{( ? )}\times\frac{24.31 g\hspace{0.2mm} Mg}{1 mol\hspace{0.2mm} Mg}\)

\(
\frac{1 mol\hspace{0.2mm} Mg}{1 mol\hspace{0.2mm} HCl}\)
\(\frac{
1 mol\hspace{0.2mm} Mg}{2 mol \hspace{0.2mm}HCl}\)
\(\frac{
(1 mol \hspace{0.2mm}MgCl_2)}{(2 mol \hspace{0.2mm}HCl)}\)
\(\frac{
(36.46 g\hspace{0.2mm} HCl)}{(1 mol\hspace{0.2mm} HCl}\)

If iron is exposed to oxygen, over time it will form iron (III) oxide \((Fe_2O_3)\), also known as rust. The reaction for this equation is represented by the equation below. When the equation is balanced, what are coefficients for Fe, \(O_2\), and \(Fe_2O_3\), respectively?

___\(Fe +\) ___\(O_2 \rightarrow\) ___\(Fe_2O_3\)

2, 1, 1
2, 3, 1
2, 3, 2
4, 3, 2

Which of the following equations is balanced?

\(3SO_2 + O_2\rightarrow 3SO_3\)
\(C_2H_6 + 5O_2 \rightarrow 2CO_2 + 3H_2O\)
\(BaCl_2 + Li_2SO_4 \rightarrow 2LiCl + BaSO_4\)
\(HNO_3 + 2Na \rightarrow 2NaNO_3 + H_2\)

The combustion reaction for butane (C₄H₁₀), the fuel inside lighters, is shown below. What coefficient must be added to oxygen (O₂) to balance this equation?

2C₄H₁₀ + ___ O₂ → 8CO₂ + 10H₂O

8
9
13
18

Which unit remains after others are canceled out in the dimensional analysis shown below?

\(\frac{(12.5 g\hspace{0.2mm} NaOH}{1}\times\frac{1 mol\hspace{0.2mm} NaOH}{40.0 g\hspace{0.2mm} NaOH}\times\frac{6.02\times10^{23} particles\hspace{0.2mm} NaOH}{1 mol\hspace{0.2mm} NaOH}=1.88\times10^{23}\)particles NaOH

g NaOH
mol NaOH
g/mol NaOH
particles NaOH

What is the molar mass of \(CuSO_4\)?

111.55 g/mol
159.55 g/mol
255.55 g/mol
446.20 g/mol

A student has attempted to balance the equation for the single-replacement reaction shown below, but it is still unbalanced. Which statement best describes how this equation is still unbalanced?

Mg + 2HCl → MgCl₂ + 2H₂

There are more chlorine atoms in the reactants.
There are more chlorine atoms in the products.
There are more hydrogen atoms in the reactants.
There are more hydrogen atoms in the products.

Silver reacts with oxygen according to the balanced equation below. How many moles of silver oxide \(Ag_2O\) are produced from 9.62 moles of silver (Ag)?

\(4Ag + O_2 \rightarrow 2Ag_2O\)

2.41 mol \(Ag_2O\)
4.81 mol \(Ag_2O\)
19.2 mol \(Ag_2O\)
38.5 mol \(Ag_2O\)

Fluorine reacts with potassium chloride (KCl) to produce potassium fluoride (KF) and chlorine gas. What mass of fluorine is required to react with 5.60 mol KCl?

\(F_2 + 2KCl \rightarrow 2KF + Cl_2\)

2.85 g F₂
53.2 g F₂
106 g F₂
213 g F₂

A water bottle contains 500 mL of water, which has a mass of 500 grams. Which conversion factor should be used to calculate the number of moles of water in the bottle?

\(\frac{1 mol\hspace{0.2mm} H_2 O}{18.02 g\hspace{0.2mm} H_2 O}\)
\(\frac{18.02 g\hspace{0.2mm} H_2 O}{1 mol\hspace{0.2mm} H_2 O}\)
\(\frac{1 mol \hspace{0.2mm}H_2 O}{6.02 \times10^{23} g\hspace{0.2mm} H_2 O}\)
\( \frac{6.02 \times10^{23} g \hspace{0.2mm}H_2 O}{1 mol \hspace{0.2mm}H_2 O}\)

The chemical equation for the synthesis of tetraphosphorus pentoxide \((P_4O_{10})\) is shown below. How many moles of oxygen \((O_2)\) are required to form 200. grams of \( (P_4O_{10})\)?

\(P4 + 5O2 \rightarrow P_4O_{10}\)

0.141 mol \(O_2\)
0.705 mol \(O_2\)
1.42 mol \(O_2\)
3.52 mol \(O_2\)

Ammonia and oxygen react to form nitrogen dioxide and water according to the chemical equation shown below. How many grams of \(NO_2\) are produced when 2.00 moles of oxygen are consumed?

\(4NH_3 + 7O_2 \rightarrow 4NO_2 + 6H_2O\)

46.0 grams
52.6 grams
105 grams
184 grams

Which question requires the following dimensional analysis?

\(\frac{(200.g \hspace{0.2mm}SCl⁡_2)}{1}\times \frac{(1 mol\hspace{0.2mm} SCl⁡_2)}{102.96 g \hspace{0.2mm}SCl⁡_2}\times\frac{6.02\times10^{23} molecules \hspace{0.2mm}SCl⁡_2}{(1 mol \hspace{0.2mm}SCl⁡_2 }=1.17\times10^{24}\) molecules \(SCl_2\)

How many grams of sulfur dichloride \( SCl_2\) were made from \(1.17 \times 10^{24}\) molecules of chlorine \((Cl_2)\)
How many moles of sulfur dichloride \(SCl_2\) have a mass of 200 grams
How many grams of sulfur dichloride \( SCl_2\) contain \(1.17 \times 10^{24}\) molecules.
How many molecules are in a 200-gram sample of sulfur dichloride \(SCl_2\)

Which equation needs to be balanced?

\(2Na + Cl_2 \rightarrow 2NaCl\)
\(2H_2O_2 \rightarrow 2H_2O + O_2\)
\(CO_2 + NO \rightarrow CO + NO_2\)
\(3Cl_2 + AlBr_3 \rightarrow AlCl_3 + 3Br_2\)

In the chemical equation below, which element is unbalanced?

\(2HNO_3 + Na \rightarrow 2NaNO_3 + H_2\)

Hydrogen
Nitrogen
Oxygen
Sodium

Which of the following compounds has the lowest molar mass?

CO
\(CO_2\)
\(H_2O\)
\(H_2O_2\)

When iron reacts with oxygen, iron (III) oxide (Fe₂O₃), also known as rust, forms according to the equation below. The iron (III) oxide has less energy than the iron and oxygen. How is reaction classified, and why?

4Fe(s) + 3O₂(g) → 2Fe₂O₃(s)

It is exothermic because energy is released.
It is exothermic because energy is absorbed.
It is endothermic because energy is released.
It is endothermic because energy is absorbed.

Which of the following equations shows a decomposition reaction?

3H₂ + N₂ → 2NH₃
2KClO₃ → 2KCl + 3O₂
2C_2H_2 + 5O₂ → 4CO₂ + 2H₂O
2Na + ZnCl₂ → Zn + 2NaCl

If 70 grams of CaCl₂ are added to 100 grams of water at 10°C, what type of mixture forms, and why?

A homogeneous mixture because all the solid will dissolve
A heterogeneous mixture because all the solid will dissolve
A homogeneous mixture because some of the solute will remain undissolved
A heterogeneous mixture because some of the solute will remain undissolved

The graph below shows the energy of the species involved in a chemical reaction as the reaction proceeds. How much energy is released in this reaction?

10 kJ
20 kJ
30 kJ
40 kJ

What is the maximum amount of KClO₃ that can be dissolved in 50 grams of water at 30°C?

5 grams
10 grams
20 grams
70 grams

Which of the following equations shows a single-replacement reaction?

3H₂ + N₂ → 2NH₃
Zn + 2HCl → H₂ + ZnCl₂
C₂H₄ + 3O₂ → 2CO₂ + 2H₂O
2AgNO₃ + CuCl₂ → 2AgCl + Cu(NO₃)₂

If barium metal (Ba) and aluminum chloride (AlCl₃) react in a single-replacement reaction, what product(s) form?

BaAlCl₃
AlBaCl₃
Al + BaCl₂
AlCl₃ + Ba

The reaction between zinc metal and hydrochloric acid (HCl) is shown below. Which product is dissolved in water at the end of the reaction?

Zn(s) + 2HCl(aq) → H₂(g) + ZnCl₂(aq)

H₂
HCl
Zn
ZnCl₂

When an antacid tablet is placed in water, fizzing is observed. The chemical equation for the reaction that occurs is shown below. Which compound is being released in the bubbles?

C₆H₈O₇(aq) + 3NaHCO₃(aq) → 3CO₂(g) + 3H₂O(l) + NaC₆H₅O₇(aq)

CO₂
H₂O
C₆H₈O₇
NaC₆H₅O₇

What type of reaction is described by the following equation?

2Na(s) + ZnCl₂(aq) → Zn(s) + 2NaCl(aq)

Synthesis
Combustion
Single-replacement
Double-replacement

What products are formed in all combustion reactions?

CH and O₂
CO₂ and O₂
H₂O and O₂
H₂O and CO₂

Which compound involved in the reaction shown below is insoluble in water?

2AgNO₃(aq) + CuCl₂(aq) → 2AgCl(s) + Cu(NO₃)₂(aq)

AgCl
AgNO₃
CuCl₂
Cu(NO₃)₂

If 30 grams of KClO₃ is added to 100 grams of water at 0°C, some of the solute remains undissolved. What is the minimum temperature that must be attained to dissolve all the solute?

30°C
70°C
80°C
100°C

Which of the following statements regarding the solubility of Ce₂(SO₄)₃ is true?

Its solubility is higher at 0°C than at 100°C.
Its solubility increases as temperature increases.
It is less soluble than all other substances in the graph below 10°C.
It is less soluble than all other substances in the graph at all temperatures.

When aqueous solutions of Pb(NO₃)₂ and KI are mixed, the reaction shown in the equation occurs, and a yellow solid appears. What is the identity of the solid?

Pb(NO₃)₂(aq)+ 2KI(aq) → PbI₂(s) + 2KNO₃(aq)

KI
PbI₂
KNO₃
Pb(NO₃)₂

In which reaction are both the reactants and the products heterogeneous mixtures?

2H₂O(g) → H₂(g) + O₂(g)
2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(g)
2AgNO₃(aq) + Cu(s) → 2Ag(s) + Cu(NO₃)₂(aq)
CaCl₂(aq) + MgSO₄(aq) → CaSO₄(s) + MgCl₂(aq)

If sulfur trioxide (SO₃) reacts with water (H₂O) in a synthesis reaction, what product(s) form?

H₂SO₄
H₂S + O₂
H₂O + SO₃
H₂O₃ + S₂O

In which reaction do the reactants form a homogeneous mixture and the products form a heterogeneous mixture?

CaO(s) + H₂O(l) → Ca(OH)₂(s)
C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g)
2Na(s) + ZnCl₂(aq) → Zn(s) → 2NaCl(aq)
Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂(s) → 2KNO₃(aq)

The equation describing the formation of ammonia (NH₃) from nitrogen and hydrogen is shown below. Which of the following statements is true?

3H₂(g) + N₂(g) → 2NH₃(g)

NH₃ is the reactant, and H₂ and N₂ are products.
H₂ and N₂ are the reactants, and NH₃ is the product.
N and H₃ are the reactants, and H₂ and N₂ are products.
H₂ and N₂ are the reactants, and N and H₃ are the products.

What type of reaction will occur between hexane (C₆H₁₄) and oxygen (O₂)?

Synthesis
Combustion
Decomposition
Single-replacement

The graph below shows the energy of the species involved in a chemical reaction as the reaction proceeds. Which of the following has the lowest amount of energy?

The products
The reactants
The transition state
The activated complex

When 15 grams of Ce₂(SO₄)₃ is added to 100 grams of water at 10 ℃, some of the solute remains undissolved. How much Ce₂(SO₄)₃ remains undissolved and settles at the bottom of the beaker?

3 grams
5 grams
8 grams
10 grams

What type of reaction is described by the following equation?

2Mg(s) + O₂(g) → 2MgO(s)

Synthesis
Decomposition
Single-replacement
Double-replacement

The graph below shows the energy of the species involved in a chemical reaction as the reaction proceeds. What is the activation energy required in this reaction?

30 kJ
40 kJ
70 kJ
100 kJ

Which of the following equations shows a double replacement reaction?

CaO + H₂O → Ca(OH)₂
2Na + ZnCl₂ → Zn(s) + 2NaCl
Pb(NO₃)₂ + 2KI → PbI₂ + 2KNO₃
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O

Inside a plant, water has to travel up, against gravity, to reach all the leaves. What property does this illustrate?

Adhesion
Bonding
Cohesion
Polarity

Why is the molecule below considered polar?

The molecule has two positive charges.
The oxygen end of the molecule is negative.
Both ends of the molecule have slight charges.
The molecule has one more positive charge than negative charge.

A solution of silver nitrate can react with small copper beads to form silver metal and a solution of copper (II) nitrate. Which of the following changes will increase the force of collisions between reactants?

\(2AgNO_3(aq) + Cu(s) \rightarrow Cu(NO_3)_2(aq) + 2Ag(s)\)

Adding water to dilute the solution of silver nitrate
Heating the reaction mixture to raise the temperature
Using a solution with a higher concentration of silver nitrate
Replacing the copper beads with smaller pieces of copper dust

For the reversible reaction shown below, which of the following statements is always true of the system at equilibrium?

\(N_2 + 3H_2 \leftrightarrow 2NH_3\)

The concentration of \(N_2\) is equal to the concentration of \(H_2\).
The concentration of \(N_2\) is equal to the concentration of \(NH_3\).
The rate of the forward reaction is equal to the rate of the reverse reaction.
The rate of the forward reaction at the beginning is equal to its rate at equilibrium.

Which of the following statements is true regarding the rates of the forward and reverse reactions for the following reversible reaction?

\(CaCO_3(s) \leftrightarrow CaO(s) + CO_2(g)\)

The rate of the forward reaction increases until the system reaches equilibrium.
The rates of the forward and reverse reactions are equal throughout the reaction.
The rates of both the forward and reverse reaction increase until the system reaches equilibrium.
The rate of the forward reaction is higher than that of the reverse reaction at the beginning of the reaction.

The energy diagram below shows two possible pathways for a reaction: one catalyzed and one uncatalyzed. Which pathway represents a reaction that will proceed faster, and why?

Pathway 1 because it has lower activation energy
Pathway 2 because it has lower activation energy
Pathway 1 because it has higher activation energy
Pathway 2 because it has higher activation energy

Two glucose molecules (\(C_6H_{12}O_6\)) react to form a molecule of maltose (\(C_{12}H_{22}O_{11}\)) and water (\(H_2O\)). The concentrations of the reactants and products are monitored, and the data is shown below. How can the data be used to determine that this is a completion rather than a reversible reaction?

\(2C_6H_{12}O_6 \rightarrow C_{12}H_{22}O_{11} + H_2O\)

\begin{array}{|c|c|c|} \hline \textbf{Time (min)} & \textbf{Concentration of Glucose (M)} & \textbf{Concentration of Maltose (M)}\\ \hline 0 &4.48 &0\\ \hline 10 &2.44 &1.02\\ \hline 20 &1.04 &1.72\\ \hline 30 &0.32 &2.08\\ \hline 40 &0.04 &2.22\\ \hline 50 &0 &2.24\\ \hline \end{array}

There is no reactant at the end of this reaction.
There is no product at the beginning of this reaction.
The amount of product increases as the reaction proceeds.
The amount of reactant decreases as the reaction proceeds.

The energy diagram below shows two possible pathways for a reaction: one catalyzed and one uncatalyzed. Which of the following is true for Pathway 1, according to the energy diagram?

It has a faster reaction rate.
It has higher activation energy.
It represents the catalyzed reaction.
It takes less time for a product to form.

How does this graph show that this reaction is reversible?

There is no product at the beginning of the reaction.
The amount of \(NO_2\) increases throughout the reaction.
There is no nitric oxide (NO) at the end of the reaction.
The concentrations of reactants and products level out.

The energy diagram below shows two possible pathways for a reaction: one catalyzed and one uncatalyzed. What does letter B represent?

The potential energy of the products
The potential energy of the reactants
The activation energy for the catalyzed reaction
The activation energy for the uncatalyzed reaction

The energy diagram below shows two possible pathways for a reaction: one catalyzed and one uncatalyzed. Which of the following is different between the catalyzed and uncatalyzed reactions?

The amount of energy released
The amount of energy required to form the transition state
The potential energy of the products at the end of the reaction
The potential energy of the reactants at the beginning of the reaction

Reaction X and Reaction Y show how fluorine (\(F_2\)) and chlorine (\(Cl_2\)) react with hydrogen (\(H_2\)). If fluorine is more reactive than chlorine, how do Reactions X and Y compare?

Reaction X: \(H_2 + F_2 \rightarrow 2HF\)
Reaction Y: \(H_2 + Cl_2 \rightarrow 2HCl\)

Reaction X will require less time than Reaction Y.
Reaction X will occur at the same rate as Reaction Y.
Reaction X will produce less product than Reaction Y.
Reaction X has the same activation energy as Reaction Y.

The graph below shows the concentrations of substances involved in a chemical reaction as the reaction progresses. Which substances are the reactants?

Only \(O_2\)
Only \(NO_2\)
\(O_2\) and NO
\(NO_2\) and NO

Which of the following statements is true regarding the role of sulfur dioxide (\(SO_2\)) in Reactions A and B?

Sulfur dioxide is a product in both Reactions A and B.
Sulfur dioxide is a reactant in both Reactions A and B.
Sulfur dioxide is a product in Reaction A and a reactant in Reaction B.
Sulfur dioxide is a reactant in Reaction A and a product in Reaction B.

An enzyme called catalase is important to many organisms because it catalyzes the decomposition of hydrogen peroxide (\(H_2O_2\)). Without this enzyme, this toxic substance would build up and damage cells. Which of the following most accurately describes how the enzyme speeds up the decomposition reaction?

Catalase causes the reaction to cool down.
Catalase causes the particles to move faster.
Catalase decreases the amount of activation energy required.
Catalase allows the particles to move farther away from each other.

The concentrations of nitrogen, hydrogen, and ammonia were monitored in a reaction, and the data is shown below. What are the products in this reaction?

\begin{array}{|c|c|c|c|} \hline \textbf{Time (min)} &\textbf{Concentration \(of H_2\) (M)} &\textbf{Concentration of \(N_2\) (M)} & \textbf{Concentration of \(NH_3\) (M)}\\ \hline 0 &1.00 &0.25 &0.0\\ \hline 10 &0.68 &0.14 &0.22\\ \hline 20 &0.49 &0.079 &0.34\\ \hline 30 &0.38 &0.041 &0.42\\ \hline 40 &0.29 &0.025 &0.45\\ \hline 50 &0.26 &0.013 &0.47\\ \hline 60 &0.25 &0.0040 &0.48\\ \hline \end{array}

Only \(H_2\)
Only \(NH_3\)
Both \(N_2\) and \(H_2\)
Both \(N_3\) and \(NH_2\)

Which of the following is true about this system at 2000 seconds?

The system has reached equilibrium.
The rates of the forward and reverse reactions are equal.
The forward reaction is proceeding more quickly than the reverse reaction.
The concentration of product is greater than the concentration of the reactants.

After the reaction below reaches equilibrium, which of the following is true?

\(H_2 + I_2 \leftrightarrow 2HI\)

Production of HI stops.
The substances \(H_2, I_2\), and HI are all being formed.
The concentration of \(H_2\) and \(I_2\) will continue to decrease.
Production of HI is a faster process than production of \(H_2\) and \(I_2\).

Hydrogen peroxide decomposes into water and oxygen, as shown in the equation below. The rate is monitored by collecting the oxygen produced and measuring its volume over time. The data table shows the volume of oxygen collected over three minutes when two catalysts, Catalyst 1 and Catalyst 2, are used. Which catalyst results in a reaction with the lower activation energy?

\(2H_2O_2(aq) \rightarrow 2H_2O(l) + O_2(g)\)

\begin{array}{|c|ccc|} \hline \textbf{Catalyst} & &\textbf{Volume of } O_2 \textbf{ collected}&\\ \hline & 1 min & 2 min & 3 min\\ \hline 1& 1.8 mL& 2.8 mL& 3.2 mL\\ \hline 2& 1.3 mL& 1.8 mL& 2.1 mL\\ \hline \end{array}

Catalyst 1 because its reaction went faster
Catalyst 2 because its reaction went faster
Catalyst 1 because its reaction went slower
Catalyst 2 because its reaction went slower

Which equation represents the reaction in the graph below?

\(2SO_3 \rightarrow 2SO_2 + O_2\)
\(2SO_2 + O_2 \rightarrow 2SO_3\)
\(2SO_3 \leftrightarrow 2SO_2 + O_2\)
\(2SO_2 + O_2 \leftrightarrow 2SO_3\)

The graph below shows the concentrations of substances involved in a chemical reaction as the reaction progresses. At what time is the reaction at equilibrium?

0 s
2000 s
3000 s
7000 s

A solution of silver nitrate can react with small copper beads to form silver metal and a solution of copper (II) nitrate. Which of the following changes will increase the frequency of collisions between reactants?

\(2AgNO_3(aq) + Cu(s) \rightarrow Cu(NO_3)_2(aq) + 2Ag(s)\)

Running the reaction in a larger reaction vessel
Cooling the reaction mixture to a lower the temperature
Increasing the concentration of the silver nitrate solution
Using one large block of solid copper rather than smaller beads

The energy diagram below shows two possible pathways for a reaction: one catalyzed and one uncatalyzed. Which of the following is the same for the catalyzed and uncatalyzed reactions?

The rate of the reaction
The potential energy of the reactants
The potential energy of the transition state
The activation energy required for the reaction to occur

Which of the following statements is true regarding Reactions A and B?

Both Reactions A and B are reversible.
Both Reactions A and B are completion reactions.
Reaction A is reversible, while Reaction B goes to completion.
Reaction A is a completion reaction, while Reaction B is reversible.

Using the periodic table, determine how many protons and electrons a neutral atom of potassium has.

19 protons, 19 electrons
19 protons, 20 electrons
19 protons, 39 electrons
39 protons, 39 electrons

Light travels at a speed of almost 3 × 10⁵ kilometers per second. How is this value written in standard notation?

0.000003 km/s
0.00003 km/s
30,000 km/s
300,000 km/s

Two silicon atoms have a length of 1 nanometer, which is equal to 1 × 10⁻⁹ meter. When this value is represented in standard notation, how many zeros are between the decimal point and the nearest non-zero digit?

7
8
9
10

The length of a year is 31,560,000 seconds. What is this value in scientific notation?

0.3156 x 10⁻⁶ s
3.156 x 10⁻⁷ s
3.156 x 10⁷ s
31.56 x 10⁶ s

An electron has a mass of 9.11 × 10⁻³¹ kg. When this value is represented in standard notation, how many zeros are between the decimal point and the nearest non-zero digit?

29
30
31
32

Which of the following numbers has the smallest magnitude?

5.14 x 10⁻²⁷
4.65 x 10⁻¹⁹
2.87 x 10⁻¹⁶
5.29 x 10⁻⁷

A nanometer is equal to 1 × 10⁻⁹ meter. How is this value written in standard notation?

0.0000000001m
0.000000001m
1,000,000,000m
10,000,000,000m

The ratio of the mass of a proton to the mass of an electron is 1,840. How is this number represented in scientific notation?

0.184 x 10⁴
1.84 x 10³
18.4 x 10²
184 x 10¹

In the heating curve for iron, at which point is the substance entirely liquid?

Point M
Point N
Point P
Point Q

Given the heating curves for fluorine, chlorine, and bromine, which halogen(s) are completely liquid at room temperature (23°C)?

Only chlorine
Only bromine
All three halogens
Both bromine and chlorine

Given the cooling curve below, what state(s) of matter were present at 10 minutes?

Solid only
Liquid only
Liquid and gas
Solid and liquid

According to the heating curve for iron, which process requires the most energy?

Boiling the entire sample
Melting the entire sample
Increasing the temperature of the solid from 0°C to the melting point
Increasing the temperature of the liquid from its melting point to its boiling point

Given the cooling curve below, what is the melting point of titanium?

500°C
1500°C
1700°C
3300°C

Given the heating curves for fluorine, chlorine, and bromine, which halogen boils at the lowest temperature?

Fluorine boils at the lowest temperature.
Chlorine boils at the lowest temperature.
Bromine boils at the lowest temperature.
They all boil at the same temperature.

At which temperature are all three halogens in the same state of matter?

-100°C
-10°C
10°C
100°C

Compare the boiling points of the alcohols in the table below. Molecules of these alcohols are similar, but they have different numbers of carbon atoms in a chain and, therefore, different masses. Based on the boiling point data in the table, what conclusion can be drawn about the relationship between the number of carbon atoms in a molecule and the interaction of the molecules?

A higher number of carbon atoms makes it more difficult for particles to stick together.
As the number of carbon atoms increases, the intermolecular forces between the particles get weaker.
A higher number of carbon atoms makes it easier for particles to spread out and move away from each other.
As the number of carbon atoms increases, the strength of the intermolecular forces between the particles increases.

Given the cooling curve below, what state(s) of matter were present between 20 and 30 minutes?

Solid only
Liquid only
Liquid and gas
Solid and liquid

Given the heating curve of iron, what are the approximate melting and boiling points?

900°C, 2300°C
1500°C, 2900°C
2300°C, 3100°C
2900°C, 3400°C

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