Question 1

The specific heat of copper is 0.385 J/(g ∙ °C).If 34.2 g of copper,initially at 24.0°C,absorbs 4.689 kJ,what will be the final temperature of the copper?

Accepted Answer

A) 24.4°C 
B) 26.8°C 
C) 356°C 
D) 380°C 
A) 24.4°C 
B) 26.8°C 
C) 356°C 
D) 380°C

Question 2

How much heat is absorbed/released when 35.00 g of NH3(g)reacts in the presence of excess O2(g)to produce NO(g)and H2O(l)according to the following chemical equation?
4 NH3(g)+ 5 O2(g)→ 4 NO(g)+ 6 H2O(l)ΔH° = 1168 kJ

Accepted Answer

A) 600.1 kJ of heat are absorbed. 
B) 600.1 kJ of heat are released. 
C) 2400 kJ of heat are absorbed. 
D) 2400 kJ of heat are released. 
A) 600.1 kJ of heat are absorbed. 
B) 600.1 kJ of heat are released. 
C) 2400 kJ of heat are absorbed. 
D) 2400 kJ of heat are released.

Question 3

The specific heat capacity of methane gas is 2.20 J/g ∙ K.How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?

Accepted Answer

A) 88.6 J 
B) 429 J 
C) 1221 J 
D) 0.0113 J 
E) 22.9 J 
A) 88.6 J 
B) 429 J 
C) 1221 J 
D) 0.0113 J 
E) 22.9 J

Question 4

How much energy is evolved during the formation of 98.7 g of Fe,according to the reaction below?
Fe2O3(s)+ 2 Al(s)→ Al2O3(s)+ 2 Fe(s)ΔH°rxn = -852 kJ

Accepted Answer

A) 753 kJ 
B) 1.51 × 103 kJ 
C) 4.20 × 103 kJ 
D) 482 kJ 
E) 241 kJ 
A) 753 kJ 
B) 1.51 × 103 kJ 
C) 4.20 × 103 kJ 
D) 482 kJ 
E) 241 kJ

Question 5

Which of the following substances (with specific heat capacity provided)would show the greatest temperature change upon absorbing 100.0 J of heat?

Accepted Answer

A) 10.0 g Cu,CCu = 0.385 J/g°C 
B) 10.0 g H2O,CH2O = 4.18 J/g°C 
C) 10.0 g ethanol,Cethanol = 2.42 J/g°C 
D) 10.0 g Al,CAl = 0.903 J/g°C 
E) 10.0 g Pb,CPb= 0.128 J/g°C 
A) 10.0 g Cu,CCu = 0.385 J/g°C 
B) 10.0 g H2O,CH2O = 4.18 J/g°C 
C) 10.0 g ethanol,Cethanol = 2.42 J/g°C 
D) 10.0 g Al,CAl = 0.903 J/g°C 
E) 10.0 g Pb,CPb= 0.128 J/g°C

Question 6

The specific heat capacity of solid copper metal is 0.385 J/g ∙ K.How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0°C to 77.5°C?

Accepted Answer

A) 1.79 × 105 J 
B) 26.6 J 
C) 2.66 × 104 J 
D) 5.58 × 10-6 J 
E) 0.00558 J 
A) 1.79 × 105 J 
B) 26.6 J 
C) 2.66 × 104 J 
D) 5.58 × 10-6 J 
E) 0.00558 J

Question 7

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction:
2 NO(g)+ O2(g)→ 2 NO2(g)ΔH°rxn = ?
Given:
N2(g)+ O2(g)→ 2 NO(g)ΔH°rxn = +183 kJ
1/2 N2(g)+ O2(g)→ NO2(g)ΔH°rxn = +33 kJ

Accepted Answer

A) -150.kJ 
B) -117 kJ 
C) -333 kJ 
D) +115 kJ 
E) +238 kJ 
A) -150.kJ 
B) -117 kJ 
C) -333 kJ 
D) +115 kJ 
E) +238 kJ

Question 8

Match the following.
--ΔE

Accepted Answer

A) work done by the system on the surroundings 
B) system gains thermal energy from surroundings 
C) energy flows out of system into the surroundings 
D) system loses thermal energy to surroundings 
E) work done on the system by the surroundings
F)energy flows into the system from the surroundings 
A) work done by the system on the surroundings 
B) system gains thermal energy from surroundings 
C) energy flows out of system into the surroundings 
D) system loses thermal energy to surroundings 
E) work done on the system by the surroundings
F)energy flows into the system from the surroundings

Question 9

For a particular process that is carried out at constant pressure,q = 145 kJ and w = -35 kJ.Therefore,

Accepted Answer

A) ΔE = 110 kJ and ΔH = 145 kJ. 
B) ΔE = 145 kJ and ΔH = 110 kJ. 
C) ΔE = 145 kJ and ΔH = 180 kJ. 
D) ΔE = 180 kJ and ΔH = 145 kJ. 
A) ΔE = 110 kJ and ΔH = 145 kJ. 
B) ΔE = 145 kJ and ΔH = 110 kJ. 
C) ΔE = 145 kJ and ΔH = 180 kJ. 
D) ΔE = 180 kJ and ΔH = 145 kJ.

Question 10

Give the equation to calculate the enthalpy of a system.

Accepted Answer

The answer of Give the equation to calculate the enthalpy...

Question 11

How much energy is evolved during the reaction of 48.7 g of Al,according to the reaction below? Assume that there is excess Fe2O3.
Fe2O3(s)+ 2 Al(s)→ Al2O3(s)+ 2 Fe(s)ΔH°rxn = -852 kJ

Accepted Answer

A) 415 kJ 
B) 207 kJ 
C) 241 kJ 
D) 130 kJ 
E) 769 kJ 
A) 415 kJ 
B) 207 kJ 
C) 241 kJ 
D) 130 kJ 
E) 769 kJ

Question 12

A 5.00-g sample of liquid water at 25.0 C is heated by the addition of 84.0 J of energy.The final temperature of the water is ________ °C.The specific heat capacity of liquid water is 4.18 J/g ∙ K.

Accepted Answer

A) 95.2 
B) 25.2 
C) -21.0 
D) 29.0 
E) 4.02 
A) 95.2 
B) 25.2 
C) -21.0 
D) 29.0 
E) 4.02

Question 13

Which of the following substances (with specific heat capacity provided)would show the greatest temperature change upon absorbing 100.0 J of heat?

Accepted Answer

A) 10.0 g Ag,CAg = 0.235 J/g°C 
B) 10.0 g H2O,CH2O = 4.18 J/g°C 
C) 10.0 g ethanol,Cethanol = 2.42 J/g°C 
D) 10.0 g Fe,CFe = 0.449 J/g°C 
E) 10.0 g Au,CAu = 0.128 J/g°C 
A) 10.0 g Ag,CAg = 0.235 J/g°C 
B) 10.0 g H2O,CH2O = 4.18 J/g°C 
C) 10.0 g ethanol,Cethanol = 2.42 J/g°C 
D) 10.0 g Fe,CFe = 0.449 J/g°C 
E) 10.0 g Au,CAu = 0.128 J/g°C

Question 14

According to the following reaction,how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g/mol.
B2H6(g)+ 6 Cl2(g)→ 2 BCl3(g)+ 6 HCl(g)ΔH°rxn = -1396 kJ

Accepted Answer

A) 1640 kJ 
B) 238 kJ 
C) 1430 kJ 
D) 3070 kJ 
E) 429 kJ 
A) 1640 kJ 
B) 238 kJ 
C) 1430 kJ 
D) 3070 kJ 
E) 429 kJ

Question 15

Using the following thermochemical equation,determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6).
2 C6H6(l)+ 15 O2(g)→ 12 CO2(g)+ 6 H2O(g)ΔH°rxn = -6278 kJ

Accepted Answer

A) 1.43 × 105 kJ/kg CO2 
B) 2.30 × 104 kJ/kg CO2 
C) 4.34 × 104 kJ/kg CO2 
D) 1.19 × 104 kJ/kg CO2 
E) 8.40 × 105 kJ/kg CO2 
A) 1.43 × 105 kJ/kg CO2 
B) 2.30 × 104 kJ/kg CO2 
C) 4.34 × 104 kJ/kg CO2 
D) 1.19 × 104 kJ/kg CO2 
E) 8.40 × 105 kJ/kg CO2

Question 16

What volume of benzene (C6H6,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 x 103 kJ of heat according to the following reaction?
2 C6H6(l)+ 15 O2(g)→ 12 CO2(g)+ 6 H2O(g)ΔH°rxn = -6278 kJ

Accepted Answer

A) 75 mL 
B) 37 mL 
C) 21 mL 
D) 19 mL 
E) 42 mL 
A) 75 mL 
B) 37 mL 
C) 21 mL 
D) 19 mL 
E) 42 mL

Question 17

At 1 atm pressure,the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol.To the correct number of significant figures,how much heat is required to melt 4.50 mol of gallium at 1 atm pressure?

Accepted Answer

A) 6 kJ 
B) 27 kJ 
C) 250 kJ 
D) 274 kJ 
A) 6 kJ 
B) 27 kJ 
C) 250 kJ 
D) 274 kJ

Question 18

How much heat is absorbed when 45.00 g of C(s)reacts in the presence of excess SO2(g)to produce CS2(l)and CO(g)according to the following chemical equation?
5 C(s)+ 2 SO2(g)→ CS2(l)+ 4 CO(g)ΔH° = 239.9 kJ

Accepted Answer

A) 179.8 kJ 
B) 239.9 kJ 
C) 898.5 kJ 
D) 2158 kJ 
A) 179.8 kJ 
B) 239.9 kJ 
C) 898.5 kJ 
D) 2158 kJ

Question 19

Determine the final temperature of a gold nugget (mass = 376 g)that starts at 398 K and loses 4.85 kJ of heat to a snowbank when it is lost.The specific heat capacity of gold is 0.128 J/g°C.

Accepted Answer

A) 133 K 
B) 398 K 
C) 187 K 
D) 297 K 
E) 377 K 
A) 133 K 
B) 398 K 
C) 187 K 
D) 297 K 
E) 377 K

Question 20

In the presence of excess oxygen,methane gas burns in a constant-pressure system to yield carbon dioxide and water:
CH4(g)+ 2O2(g)→ CO2(g)+ 2H2O(l)ΔH = -890.0 kJ
Calculate the value of q (kJ)in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

Accepted Answer

A) -94.6 kJ 
B) 0.0306 kJ 
C) -0.0106 kJ 
D) 32.7 kJ 
E) -9.46 × 104 kJ 
A) -94.6 kJ 
B) 0.0306 kJ 
C) -0.0106 kJ 
D) 32.7 kJ 
E) -9.46 × 104 kJ

The specific heat of copper is 0.385 J/(g ∙ °C).If 34.2 g of copper,initially at 24.0°C,absorbs 4.689 kJ,what will be the final temperature of the copper?

How much heat is absorbed/released when 35.00 g of NH₃(g)reacts in the presence of excess O₂(g)to produce NO(g)and H₂O(l)according to the following chemical equation? 4 NH₃(g)+ 5 O₂(g)→ 4 NO(g)+ 6 H₂O(l)ΔH° = 1168 kJ

The specific heat capacity of methane gas is 2.20 J/g ∙ K.How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?

How much energy is evolved during the formation of 98.7 g of Fe,according to the reaction below? Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)ΔH°_rxn= -852 kJ

Which of the following substances (with specific heat capacity provided)would show the greatest temperature change upon absorbing 100.0 J of heat?

The specific heat capacity of solid copper metal is 0.385 J/g ∙ K.How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0°C to 77.5°C?

Use the standard reaction enthalpies given below to determine ΔH°_rxn for the following reaction: 2 NO(g)+ O₂(g)→ 2 NO₂(g)ΔH°_rxn= ? Given: N₂(g)+ O₂(g)→ 2 NO(g)ΔH°_rxn= +183 kJ 1/2 N₂(g)+ O₂(g)→ NO₂(g)ΔH°_rxn= +33 kJ

Match the following. --ΔE

For a particular process that is carried out at constant pressure,q = 145 kJ and w = -35 kJ.Therefore,

Give the equation to calculate the enthalpy of a system.

How much energy is evolved during the reaction of 48.7 g of Al,according to the reaction below? Assume that there is excess Fe₂O₃. Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)ΔH°_rxn= -852 kJ

A 5.00-g sample of liquid water at 25.0 C is heated by the addition of 84.0 J of energy.The final temperature of the water is ________ °C.The specific heat capacity of liquid water is 4.18 J/g ∙ K.

Which of the following substances (with specific heat capacity provided)would show the greatest temperature change upon absorbing 100.0 J of heat?

According to the following reaction,how much energy is evolved during the reaction of 32.5 g B₂H₆ and 72.5 g Cl₂? The molar mass of B₂H₆is 27.67 g/mol. B₂H₆(g)+ 6 Cl₂(g)→ 2 BCl₃(g)+ 6 HCl(g)ΔH°_rxn= -1396 kJ

Using the following thermochemical equation,determine the amount of heat produced per kg of CO₂ formed during the combustion of benzene (C₆H₆). 2 C₆H₆(l)+ 15 O₂(g)→ 12 CO₂(g)+ 6 H₂O(g)ΔH°_rxn= -6278 kJ

What volume of benzene (C₆H₆,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 x 10³ kJ of heat according to the following reaction? 2 C₆H₆(l)+ 15 O₂(g)→ 12 CO₂(g)+ 6 H₂O(g)ΔH°_rxn= -6278 kJ

At 1 atm pressure,the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol.To the correct number of significant figures,how much heat is required to melt 4.50 mol of gallium at 1 atm pressure?

How much heat is absorbed when 45.00 g of C(s)reacts in the presence of excess SO₂(g)to produce CS₂(l)and CO(g)according to the following chemical equation? 5 C(s)+ 2 SO₂(g)→ CS₂(l)+ 4 CO(g)ΔH° = 239.9 kJ

Determine the final temperature of a gold nugget (mass = 376 g)that starts at 398 K and loses 4.85 kJ of heat to a snowbank when it is lost.The specific heat capacity of gold is 0.128 J/g°C.

In the presence of excess oxygen,methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH₄(g)+ 2O₂(g)→ CO₂(g)+ 2H₂O(l)ΔH = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

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Exam 6: Thermochemistry

The specific heat of copper is 0.385 J/(g ∙ °C).If 34.2 g of copper,initially at 24.0°C,absorbs 4.689 kJ,what will be the final temperature of the copper?

How much heat is absorbed/released when 35.00 g of NH3(g)reacts in the presence of excess O2(g)to produce NO(g)and H2O(l)according to the following chemical equation? 4 NH3(g)+ 5 O2(g)→ 4 NO(g)+ 6 H2O(l)ΔH° = 1168 kJ

The specific heat capacity of methane gas is 2.20 J/g ∙ K.How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?

How much energy is evolved during the formation of 98.7 g of Fe,according to the reaction below? Fe2O3(s)+ 2 Al(s)→ Al2O3(s)+ 2 Fe(s)ΔH°rxn = -852 kJ

Which of the following substances (with specific heat capacity provided)would show the greatest temperature change upon absorbing 100.0 J of heat?

The specific heat capacity of solid copper metal is 0.385 J/g ∙ K.How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0°C to 77.5°C?

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 2 NO(g)+ O2(g)→ 2 NO2(g)ΔH°rxn = ? Given: N2(g)+ O2(g)→ 2 NO(g)ΔH°rxn = +183 kJ 1/2 N2(g)+ O2(g)→ NO2(g)ΔH°rxn = +33 kJ

Match the following. --ΔE

For a particular process that is carried out at constant pressure,q = 145 kJ and w = -35 kJ.Therefore,

Give the equation to calculate the enthalpy of a system.

How much energy is evolved during the reaction of 48.7 g of Al,according to the reaction below? Assume that there is excess Fe2O3. Fe2O3(s)+ 2 Al(s)→ Al2O3(s)+ 2 Fe(s)ΔH°rxn = -852 kJ

A 5.00-g sample of liquid water at 25.0 C is heated by the addition of 84.0 J of energy.The final temperature of the water is ________ °C.The specific heat capacity of liquid water is 4.18 J/g ∙ K.

Which of the following substances (with specific heat capacity provided)would show the greatest temperature change upon absorbing 100.0 J of heat?

According to the following reaction,how much energy is evolved during the reaction of 32.5 g B2H6 and 72.5 g Cl2? The molar mass of B2H6 is 27.67 g/mol. B2H6(g)+ 6 Cl2(g)→ 2 BCl3(g)+ 6 HCl(g)ΔH°rxn = -1396 kJ

Using the following thermochemical equation,determine the amount of heat produced per kg of CO2 formed during the combustion of benzene (C6H6). 2 C6H6(l)+ 15 O2(g)→ 12 CO2(g)+ 6 H2O(g)ΔH°rxn = -6278 kJ

What volume of benzene (C6H6,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 x 103 kJ of heat according to the following reaction? 2 C6H6(l)+ 15 O2(g)→ 12 CO2(g)+ 6 H2O(g)ΔH°rxn = -6278 kJ

At 1 atm pressure,the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol.To the correct number of significant figures,how much heat is required to melt 4.50 mol of gallium at 1 atm pressure?

How much heat is absorbed when 45.00 g of C(s)reacts in the presence of excess SO2(g)to produce CS2(l)and CO(g)according to the following chemical equation? 5 C(s)+ 2 SO2(g)→ CS2(l)+ 4 CO(g)ΔH° = 239.9 kJ

Determine the final temperature of a gold nugget (mass = 376 g)that starts at 398 K and loses 4.85 kJ of heat to a snowbank when it is lost.The specific heat capacity of gold is 0.128 J/g°C.

In the presence of excess oxygen,methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g)+ 2O2(g)→ CO2(g)+ 2H2O(l)ΔH = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

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How much heat is absorbed/released when 35.00 g of NH₃(g)reacts in the presence of excess O₂(g)to produce NO(g)and H₂O(l)according to the following chemical equation? 4 NH₃(g)+ 5 O₂(g)→ 4 NO(g)+ 6 H₂O(l)ΔH° = 1168 kJ

How much energy is evolved during the formation of 98.7 g of Fe,according to the reaction below? Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)ΔH°_rxn= -852 kJ

Use the standard reaction enthalpies given below to determine ΔH°_rxn for the following reaction: 2 NO(g)+ O₂(g)→ 2 NO₂(g)ΔH°_rxn= ? Given: N₂(g)+ O₂(g)→ 2 NO(g)ΔH°_rxn= +183 kJ 1/2 N₂(g)+ O₂(g)→ NO₂(g)ΔH°_rxn= +33 kJ

How much energy is evolved during the reaction of 48.7 g of Al,according to the reaction below? Assume that there is excess Fe₂O₃. Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)ΔH°_rxn= -852 kJ

According to the following reaction,how much energy is evolved during the reaction of 32.5 g B₂H₆ and 72.5 g Cl₂? The molar mass of B₂H₆is 27.67 g/mol. B₂H₆(g)+ 6 Cl₂(g)→ 2 BCl₃(g)+ 6 HCl(g)ΔH°_rxn= -1396 kJ

Using the following thermochemical equation,determine the amount of heat produced per kg of CO₂ formed during the combustion of benzene (C₆H₆). 2 C₆H₆(l)+ 15 O₂(g)→ 12 CO₂(g)+ 6 H₂O(g)ΔH°_rxn= -6278 kJ

What volume of benzene (C₆H₆,d= 0.88 g/mL,molar mass = 78.11 g/mol)is required to produce 1.5 x 10³ kJ of heat according to the following reaction? 2 C₆H₆(l)+ 15 O₂(g)→ 12 CO₂(g)+ 6 H₂O(g)ΔH°_rxn= -6278 kJ

How much heat is absorbed when 45.00 g of C(s)reacts in the presence of excess SO₂(g)to produce CS₂(l)and CO(g)according to the following chemical equation? 5 C(s)+ 2 SO₂(g)→ CS₂(l)+ 4 CO(g)ΔH° = 239.9 kJ

In the presence of excess oxygen,methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH₄(g)+ 2O₂(g)→ CO₂(g)+ 2H₂O(l)ΔH = -890.0 kJ Calculate the value of q (kJ)in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.