Question 1

A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper?

Accepted Answer

A) 0.385 J/g·°C 
B) 1.83 * 104 J/g·°C 
C) 2.60 J/g·°C 
D) 1.32 J/g·°C 
E) 24.5 J/g·°C 
A) 0.385 J/g·°C 
B) 1.83 * 104 J/g·°C 
C) 2.60 J/g·°C 
D) 1.32 J/g·°C 
E) 24.5 J/g·°C

Question 2

The combustion of one mole of benzene, C6H6, in oxygen liberates 3268 kJ of heat. The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

Accepted Answer

Question 3

A gas is compressed in a cylinder from a volume of 20.0 L to 2.0 L by a constant pressure of 10.0 atm. Calculate the amount of work done on the system.

Accepted Answer

A) 1.01 * 104 J 
B) -180 J 
C) 1.81 * 104 J 
D) -1.81 * 104 J 
E) 180 J 
A) 1.01 * 104 J 
B) -180 J 
C) 1.81 * 104 J 
D) -1.81 * 104 J 
E) 180 J

Question 4

Given the following $\Delta$H° values,
H2(g)+   O2(g)$\rarr$ H2O(l)$\Delta$H°f = -285.8 kJ/mol
H2O2(l)$\rarr$ H2(g)+ O2(g)$\Delta$H°rxn = 187.6 kJ/mol
calculate $\Delta$H°rxn for the reaction H2O2(l)$\rarr$H2O(l)+   O2(g),

Accepted Answer

The answer of Given the following $\Delta$H° values,
H2(g)+  ...

Question 5

The heat released when one mole of water is formed from the elements is 1,198 kJ. An experiment was conducted that permitted water to form in this manner, and the heat was contained in 2.0 liters of water. The water temperature before the reaction was 34.5°C, and after the reaction it had risen to 52.0°C. How many moles of water were formed? (The specific heat of water is 4.184 J/g·°C.)

Accepted Answer

The answer of The heat released when one mole of...

Question 6

The heat of combustion of propane, C3H8, 2220 kJ/mol. The specific heat of copper is 0.385 J/g.°C. How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings?

Accepted Answer

The answer of The heat of combustion of propane, C3H8,...

Question 7

A 0.1946 g piece of magnesium metal is burned in a constant-volume calorimeter that has a heat capacity of 1349 J/°C. The calorimeter contains 500. g of water and the temperature rise is 1.40°C. Calculate the heat of combustion of magnesium metal in kJ/g, given that the specific heat of water = 4.184 J/g·°C.

Accepted Answer

The answer of A 0.1946 g piece of magnesium metal...

Question 8

If 2Mg(s)+ O2(g)$\rarr$2MgO(s), $\Delta$H° = -1203.6 kJ/mol.
For Mg(s)+ (1/2)O2(g)$\rarr$ MgO(s), the enthalpy change is $\Delta$H = -601.8 kJ/mol.

Accepted Answer

A) True 
 B)False

Question 9

Thermal energy is

Accepted Answer

A) the energy stored within the structural units of chemical substances. 
B) the energy associated with the random motion of atoms and molecules. 
C) solar energy, i.e. energy that comes from the sun. 
D) energy available by virtue of an object's position. 
A) the energy stored within the structural units of chemical substances. 
B) the energy associated with the random motion of atoms and molecules. 
C) solar energy, i.e. energy that comes from the sun. 
D) energy available by virtue of an object's position.

Question 10

Find $\Delta$H°rxn for the reaction
2Na(s)+ 2H2O(l)$\rarr$2NaOH(aq)+ 2H2(g).
[$\Delta$H°f (NaOH(aq))= -426.8 kJ/mol; $\Delta$H°f (H2O(l))= -285.5 kJ/mol]

Accepted Answer

The answer of Find $\Delta$H°rxn for the reaction
2Na(s)+ 2H2O(l)$\rarr$2NaOH(aq)+ 2H2(g).
[$\Delta$H°f...

Question 11

The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH4NO3 is added to 40.0 mL of water in a calorimeter at 23.5°C, what is the minimum temperature reached by the solution? (The specific heat of water = 4.18 J/g·°C; the heat capacity of the calorimeter = 650. J/°C.)

Accepted Answer

A) 14.3°C 
B) 20.8°C 
C) -7.7°C 
D) 25.6°C 
E) 21.4°C 
A) 14.3°C 
B) 20.8°C 
C) -7.7°C 
D) 25.6°C 
E) 21.4°C

Question 12

The combustion of butane produces heat according to the equation 2C4H10(g)+ 13O2(g)$\rarr$8CO2(g)+ 10H2O(l)$\Delta$H°rxn = -5,314 kJ/mol
What is the heat of combustion per gram of butane?

Accepted Answer

A) -32.5 kJ/g 
B) -45.7 kJ/g 
C) -91.5 kJ/g 
D) -2,656 kJ/g 
E) -15,440 kJ/g 
A) -32.5 kJ/g 
B) -45.7 kJ/g 
C) -91.5 kJ/g 
D) -2,656 kJ/g 
E) -15,440 kJ/g

Question 13

The combustion of octane produces heat according to the equation 2C8H18(l)+ 25O2(g)$\rarr$16CO2(g)+ 18H2O(l)$\Delta$H°rxn= -11,020 kJ/mol
What is the heat of combustion per gram of octane?

Accepted Answer

A) -5,510 kJ/g 
B) -96.5 kJ/g 
C) -48.2 kJ/g 
D) -193 kJ/g 
E) -6.292 * 105 kJ/g 
A) -5,510 kJ/g 
B) -96.5 kJ/g 
C) -48.2 kJ/g 
D) -193 kJ/g 
E) -6.292 * 105 kJ/g

Question 14

A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/°C. If the temperature rise of the calorimeter with water was 0.570°C, calculate the enthalpy of combustion of magnesium. Mg(s)+ 1/2O2(g)$\rarr$ MgO(s)

Accepted Answer

A) -3280 kJ/mol 
B) -24.8 kJ/mol 
C) 435 kJ/mol 
D) 106 kJ/mol 
E) -602 kJ/mol 
A) -3280 kJ/mol 
B) -24.8 kJ/mol 
C) 435 kJ/mol 
D) 106 kJ/mol 
E) -602 kJ/mol

Question 15

A 100. mL sample of 0.200 M aqueous hydrochloric acid is added to 100. mL of 0.200 M aqueous ammonia in a calorimeter whose heat capacity (excluding any water)is 480. J/K. The following reaction occurs when the two solutions are mixed. HCl(aq)+ NH3(aq)$\rarr$NH4Cl(aq)
The temperature increase is 2.34°C. Calculate $\Delta$H per mole of HCl and NH3 reacted.

Accepted Answer

A) 154 kJ/mol 
B) 1.96 kJ/mol 
C) 485 kJ/mol 
D) -1.96 kJ/mol 
E) -154 kJ/mol 
A) 154 kJ/mol 
B) 1.96 kJ/mol 
C) 485 kJ/mol 
D) -1.96 kJ/mol 
E) -154 kJ/mol

Question 16

Find the heat absorbed from the surroundings when 15 g of O2 reacts according to the equation O + O2 $\rarr$ O3, $\Delta$H°rxn= -103 kJ/mol.

Accepted Answer

A) 4.6 * 10-3 kJ 
B) 48 kJ 
C) 96 kJ 
D) 32 kJ 
E) 110 kJ 
A) 4.6 * 10-3 kJ 
B) 48 kJ 
C) 96 kJ 
D) 32 kJ 
E) 110 kJ

Question 17

Naphthalene combustion can be used to calibrate the heat capacity of a bomb calorimeter. The heat of combustion of naphthalene is -40.1 kJ/g. When 0.8210 g of naphthalene was burned in a calorimeter containing 1,000. g of water, a temperature rise of 4.21°C was observed. What is the heat capacity of the bomb calorimeter excluding the water?

Accepted Answer

A) 32.9 kJ/°C 
B) 7.8 kJ/°C 
C) 3.64 kJ/°C 
D) 1.76 kJ/°C 
E) 15.3 kJ/°C 
A) 32.9 kJ/°C 
B) 7.8 kJ/°C 
C) 3.64 kJ/°C 
D) 1.76 kJ/°C 
E) 15.3 kJ/°C

Question 18

Define specific heat.

Accepted Answer

The amount of heat required to

Question 19

Calcium oxide and water react in an exothermic reaction: CaO(s)+ H2O(l)$\rarr$ Ca(OH)2(s)$\Delta$H°rxn = -64.8 kJ/mol
How much heat would be liberated when 7.15 g CaO(s)is dropped into a beaker containing 152g H2O?

Accepted Answer

A) 1.97 * 10-3 kJ 
B) 8.26 kJ 
C) 508 kJ 
D) 547 kJ 
E) 555 kJ 
A) 1.97 * 10-3 kJ 
B) 8.26 kJ 
C) 508 kJ 
D) 547 kJ 
E) 555 kJ

Question 20

Ethanol (C2H5OH)burns according to the equation C2H5OH(l)+ 3O2(g)$\rarr$ 2CO2(g)+ 3H2O(l), $\Delta$H°rxn = -1367 kJ/mol.
How much heat is released when 35.0 g of ethanol is burned?

Accepted Answer

A) 1,797 kJ 
B) 1,367 kJ 
C) 9.61 * 10-4 kJ 
D) 4.78 * 104 kJ 
E) 1,040 kJ 
A) 1,797 kJ 
B) 1,367 kJ 
C) 9.61 * 10-4 kJ 
D) 4.78 * 104 kJ 
E) 1,040 kJ

A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper?

The combustion of one mole of benzene, C₆H₆, in oxygen liberates 3268 kJ of heat. The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

A gas is compressed in a cylinder from a volume of 20.0 L to 2.0 L by a constant pressure of 10.0 atm. Calculate the amount of work done on the system.

The heat of combustion of propane, C₃H₈, 2220 kJ/mol. The specific heat of copper is 0.385 J/g.°C. How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings?

If 2Mg(s)+ O₂(g) $\rarr$ 2MgO(s), $\Delta$ H° = -1203.6 kJ/mol. For Mg(s)+ (1/2)O₂(g) $\rarr$ MgO(s), the enthalpy change is $\Delta$ H = -601.8 kJ/mol.

Thermal energy is

Find $\Delta$ H°_rxn for the reaction 2Na(s)+ 2H₂O(l) $\rarr$ 2NaOH(aq)+ 2H₂(g). [ $\Delta$ H°_f (NaOH(aq))= -426.8 kJ/mol; $\Delta$ H°_f (H₂O(l))= -285.5 kJ/mol]

The combustion of butane produces heat according to the equation 2C₄H₁₀(g)+ 13O₂(g) $\rarr$ 8CO₂(g)+ 10H₂O(l) $\Delta$ H°_rxn = -5,314 kJ/mol What is the heat of combustion per gram of butane?

The combustion of octane produces heat according to the equation 2C₈H₁₈(l)+ 25O₂(g) $\rarr$ 16CO₂(g)+ 18H₂O(l) $\Delta$ H°_rxn= -11,020 kJ/mol What is the heat of combustion per gram of octane?

A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/°C. If the temperature rise of the calorimeter with water was 0.570°C, calculate the enthalpy of combustion of magnesium. Mg(s)+ 1/2O₂(g) $\rarr$ MgO(s)

Find the heat absorbed from the surroundings when 15 g of O₂ reacts according to the equation O + O₂ $\rarr$ O₃, $\Delta$ H°_rxn= -103 kJ/mol.

Define specific heat.

Calcium oxide and water react in an exothermic reaction: CaO(s)+ H₂O(l) $\rarr$ Ca(OH)₂(s) $\Delta$ H°_rxn = -64.8 kJ/mol How much heat would be liberated when 7.15 g CaO(s)is dropped into a beaker containing 152g H₂O?

Ethanol (C₂H₅OH)burns according to the equation C₂H₅OH(l)+ 3O₂(g) $\rarr$ 2CO₂(g)+ 3H₂O(l), $\Delta$ H°_rxn = -1367 kJ/mol. How much heat is released when 35.0 g of ethanol is burned?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

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Exam 6: Energy Relationships in Chemical Reactions

A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper?

The combustion of one mole of benzene, C6H6, in oxygen liberates 3268 kJ of heat. The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

A gas is compressed in a cylinder from a volume of 20.0 L to 2.0 L by a constant pressure of 10.0 atm. Calculate the amount of work done on the system.

Given the following Δ\DeltaΔ H° values, H2(g)+ O2(g) →\rarr→ H2O(l) Δ\DeltaΔ H°f = -285.8 kJ/mol H2O2(l) →\rarr→ H2(g)+ O2(g) Δ\DeltaΔ H°rxn = 187.6 kJ/mol calculate Δ\DeltaΔ H°rxn for the reaction H2O2(l) →\rarr→ H2O(l)+ O2(g),

The heat of combustion of propane, C3H8, 2220 kJ/mol. The specific heat of copper is 0.385 J/g.°C. How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings?

If 2Mg(s)+ O2(g) →\rarr→ 2MgO(s), Δ\DeltaΔ H° = -1203.6 kJ/mol. For Mg(s)+ (1/2)O2(g) →\rarr→ MgO(s), the enthalpy change is Δ\DeltaΔ H = -601.8 kJ/mol.

Thermal energy is

Find Δ\DeltaΔ H°rxn for the reaction 2Na(s)+ 2H2O(l) →\rarr→ 2NaOH(aq)+ 2H2(g). [ Δ\DeltaΔ H°f (NaOH(aq))= -426.8 kJ/mol; Δ\DeltaΔ H°f (H2O(l))= -285.5 kJ/mol]

The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH4NO3 is added to 40.0 mL of water in a calorimeter at 23.5°C, what is the minimum temperature reached by the solution? (The specific heat of water = 4.18 J/g·°C; the heat capacity of the calorimeter = 650. J/°C.)

The combustion of butane produces heat according to the equation 2C4H10(g)+ 13O2(g) →\rarr→ 8CO2(g)+ 10H2O(l) Δ\DeltaΔ H°rxn = -5,314 kJ/mol What is the heat of combustion per gram of butane?

The combustion of octane produces heat according to the equation 2C8H18(l)+ 25O2(g) →\rarr→ 16CO2(g)+ 18H2O(l) Δ\DeltaΔ H°rxn= -11,020 kJ/mol What is the heat of combustion per gram of octane?

A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/°C. If the temperature rise of the calorimeter with water was 0.570°C, calculate the enthalpy of combustion of magnesium. Mg(s)+ 1/2O2(g) →\rarr→ MgO(s)

Find the heat absorbed from the surroundings when 15 g of O2 reacts according to the equation O + O2 →\rarr→ O3, Δ\DeltaΔ H°rxn= -103 kJ/mol.

Define specific heat.

Calcium oxide and water react in an exothermic reaction: CaO(s)+ H2O(l) →\rarr→ Ca(OH)2(s) Δ\DeltaΔ H°rxn = -64.8 kJ/mol How much heat would be liberated when 7.15 g CaO(s)is dropped into a beaker containing 152g H2O?

Ethanol (C2H5OH)burns according to the equation C2H5OH(l)+ 3O2(g) →\rarr→ 2CO2(g)+ 3H2O(l), Δ\DeltaΔ H°rxn = -1367 kJ/mol. How much heat is released when 35.0 g of ethanol is burned?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

The combustion of one mole of benzene, C₆H₆, in oxygen liberates 3268 kJ of heat. The products of the reaction are carbon dioxide and water. How much heat is given off when 183 g of oxygen are reacted with excess benzene?

The heat of combustion of propane, C₃H₈, 2220 kJ/mol. The specific heat of copper is 0.385 J/g.°C. How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings?

If 2Mg(s)+ O₂(g) $\rarr$ 2MgO(s), $\Delta$ H° = -1203.6 kJ/mol. For Mg(s)+ (1/2)O₂(g) $\rarr$ MgO(s), the enthalpy change is $\Delta$ H = -601.8 kJ/mol.

Find $\Delta$ H°_rxn for the reaction 2Na(s)+ 2H₂O(l) $\rarr$ 2NaOH(aq)+ 2H₂(g). [ $\Delta$ H°_f (NaOH(aq))= -426.8 kJ/mol; $\Delta$ H°_f (H₂O(l))= -285.5 kJ/mol]

The combustion of butane produces heat according to the equation 2C₄H₁₀(g)+ 13O₂(g) $\rarr$ 8CO₂(g)+ 10H₂O(l) $\Delta$ H°_rxn = -5,314 kJ/mol What is the heat of combustion per gram of butane?

The combustion of octane produces heat according to the equation 2C₈H₁₈(l)+ 25O₂(g) $\rarr$ 16CO₂(g)+ 18H₂O(l) $\Delta$ H°_rxn= -11,020 kJ/mol What is the heat of combustion per gram of octane?

A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/°C. If the temperature rise of the calorimeter with water was 0.570°C, calculate the enthalpy of combustion of magnesium. Mg(s)+ 1/2O₂(g) $\rarr$ MgO(s)

Find the heat absorbed from the surroundings when 15 g of O₂ reacts according to the equation O + O₂ $\rarr$ O₃, $\Delta$ H°_rxn= -103 kJ/mol.

Calcium oxide and water react in an exothermic reaction: CaO(s)+ H₂O(l) $\rarr$ Ca(OH)₂(s) $\Delta$ H°_rxn = -64.8 kJ/mol How much heat would be liberated when 7.15 g CaO(s)is dropped into a beaker containing 152g H₂O?

Ethanol (C₂H₅OH)burns according to the equation C₂H₅OH(l)+ 3O₂(g) $\rarr$ 2CO₂(g)+ 3H₂O(l), $\Delta$ H°_rxn = -1367 kJ/mol. How much heat is released when 35.0 g of ethanol is burned?