Question 1

It takes 18.2 kJ of energy to raise the temperature of 55.2g of an unknown liquid from 30.0°C to 47.0°C.What is the specific heat of the unknown liquid

Accepted Answer

A)   1. 17 J/(g ∙ °
C)  
B)   205J/(g ∙ °
C)  
C)   89.0 J/(g ∙ °
C)  
D)   19.4 J/(g ∙ °
C)   D

Question 2

Energy that is associated with the relative positions of electrons and nuclei in atoms and molecules is called

Accepted Answer

A)   kinetic energy.
B)   thermal energy.
C)   gravitational energy.
D)   chemical energy.

Question 3

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

Question 4

Which one of the following elements is NOT in its standard state?

Accepted Answer

A)   Br2(g) 
B)   F2(g) 
C)   Hg(l) 
D)   Na(s) 
E)   Cl2(g)

Question 5

Which of the following processes are endothermic?

Accepted Answer

A)   the reaction associated with the lattice energy of LiCl
B)   the reaction associated with the ionization energy of potassium
C)   the reaction associated with the heat of formation of CaS
D)   the formation of F2 from its elements in their standard states
E)   None of the above are endothermic.

Question 6

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

Accepted Answer

A)   4.38 J/g°C
B)   2.29 J/g°C
C)   3.95 J/g°C
D)   2.53 J/g°C
E)   1.87 J/g°C

Question 7

If a block of gold requires 1.42 kJ of energy to raise the temperature from 120.0°C to 240.0°C,what is the mass of the block? The specific heat capacity of gold is 0.129 J/g-K.

Accepted Answer

A)   92.0 g
B)   35.3 g
C)   186 g
D)   55.7 g

Question 8

Use the bond energies provided to estimate ΔH°rxn for the reaction below. CH3OH(l) + 2 O2(g) → CO2(g) + 2 H2O(g) ΔH°rxn = ?
Bond Bond Energy (kJ/mol) 
C-H 414
C-O 360
C=O 799
O=O 498
O-H 464

Accepted Answer

A)   +473 kJ
B)   -91 kJ
C)   -486 kJ
D)   -392 kJ
E)   +206 kJ

Question 9

Give the units of heat capacity.

Accepted Answer

A)   J/°C
B)   J/g °C
C)   Jmole/°C
D)   g/°C
E)   mole/°C

Question 10

Choose the reaction that illustrates ΔH°f for Mg(NO3) 2.

Accepted Answer

A)   Mg(s)  + N2(g)  + 3O2(g)  → Mg(NO3) 2(s) 
B)   Mg2+(aq)  + 2 NO3-(aq)  → Mg(NO3) 2(aq) 
C)   Mg(s)  + 2 N(g)  + 6 O(g)  → Mg(NO3) 2(s) 
D)   Mg(NO3) 2(aq)  → Mg2+(aq)  + 2 NO3-(aq) 
E)   Mg(NO3) 2(s)  → Mg(s)  + N2(g)  + 3O2(g)

Question 11

Where does the energy absorbed during an endothermic reaction go?

Accepted Answer

During an endothermic reaction,the produ...

Question 12

When 10.00 moles of H2(g) reacts with 5.000 mol of O2(g) to form 10.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm.If 683.0 kJ of heat are released during this reaction,and PΔV is equal to -37.00 kJ,then

Accepted Answer

A)   ΔH° = +683.0 kJ and ΔE° = +720.0 kJ.
B)   ΔH° = +683.0 kJ and ΔE° = +646.0 kJ.
C)   ΔH° = -683.0 kJ and ΔE° = -646.0 kJ.
D)   ΔH° = -683.0 kJ and ΔE° = -720.0 kJ.

Question 13

According to the following thermochemical equation,what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO2.
SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ

Accepted Answer

A)   42.7 g
B)   37.5 g
C)   150. g
D)   107 g
E)   173 g

Question 14

Which of the following statements is TRUE?

Accepted Answer

A)   State functions do not depend on the path taken to arrive at a particular state.
B)   DErxn can be determined using constant volume calorimetry.
C)   Energy is neither created nor destroyed, excluding nuclear reactions.
D)   ΔHrxn can be determined using constant pressure calorimetry.
E)   All of the above are true. E

Question 15

At 1 atm pressure,the heat of sublimation of gallium is 277.0kJ/mol and the heat of vaporization is 271.0 kJ/mol.To the correct number of significant figures,how much heat is required to melt 5.50 mol of gallium at 1 atm pressure?

Accepted Answer

A)   6 kJ
B)   33 kJ
C)   244 kJ
D)   274 kJ B

Question 16

The combustion of titanium with oxygen produces titanium dioxide: Ti(s) +  (g) →  (s) 
When 2.060 g of titanium is combusted in a bomb calorimeter,the temperature of the calorimeter increases from 25.00°C to 91.60°C.In a separate experiment,the heat capacity of the calorimeter is measured to be 9.84 kJ/K.The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ/mol.

Accepted Answer

A)   14.3
B)   19.6
C)   -311
D)   -0.154
E)   -1.52 ×

Question 17

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g)  ΔH°f (kJ/mol)  2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJ
SO2(g) -297

Accepted Answer

A)   -792 kJ/mol
B)   -248 kJ/mol
C)   -495 kJ/mol
D)   -578 kJ/mol
E)   -396 kJ/mol

Question 18

Which of the following processes is endothermic?

Accepted Answer

A)   the freezing of water
B)   the combustion of butane
C)   a hot cup of coffee (system)  cools on a countertop
D)   the chemical reaction in a "hot pack" often used to treat sore muscles
E)   the vaporization of rubbing alcohol

Question 19

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF ΔH°f (kJ/mol)  IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ
IF7(g) 941
IF5(g) 840

Accepted Answer

A)   101 kJ/mol
B)   -146 kJ/mol
C)   -190. kJ/mol
D)   -95 kJ/mol
E)   24 kJ/mol

Question 20

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/ml by 7.80°C? (The specific heat of the solution is 3.74 J/g∙K.)

Accepted Answer

A)   -7.43 kJ
B)   -12.51 kJ
C)   8.20 kJ
D)   -9.12 kJ
E)   6.51 kJ

Exam 10: Thermochemistry

It takes 18.2 kJ of energy to raise the temperature of 55.2g of an unknown liquid from 30.0°C to 47.0°C.What is the specific heat of the unknown liquid

Correct Answer
verified
D

Energy that is associated with the relative positions of electrons and nuclei in atoms and molecules is called

Correct Answer
verified

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

Correct Answer
verified

Which one of the following elements is NOT in its standard state?

Correct Answer
verified

Which of the following processes are endothermic?

Correct Answer
verified

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

Correct Answer
verified

If a block of gold requires 1.42 kJ of energy to raise the temperature from 120.0°C to 240.0°C,what is the mass of the block? The specific heat capacity of gold is 0.129 J/g-K.

Correct Answer
verified

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. CH₃OH(l) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) ΔH°_rxn= ? Bond Bond Energy (kJ/mol) C-H 414 C-O 360 C=O 799 O=O 498 O-H 464

Correct Answer
verified

Give the units of heat capacity.

Correct Answer
verified

Choose the reaction that illustrates ΔH°_f for Mg(NO₃) ₂.

Correct Answer
verified

Where does the energy absorbed during an endothermic reaction go?

Correct Answer
verified
During an endothermic reaction,the produ...
View Answer

When 10.00 moles of H₂(g) reacts with 5.000 mol of O₂(g) to form 10.00 mol of H₂O(l) at 25°C and a constant pressure of 1.00 atm.If 683.0 kJ of heat are released during this reaction,and PΔV is equal to -37.00 kJ,then

Correct Answer
verified

According to the following thermochemical equation,what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO₂. SiO₂(s) + 4 HF(g) → SiF₄(g) + 2 H₂O(l) ΔH°_rxn= -184 kJ

Correct Answer
verified

Which of the following statements is TRUE?

Correct Answer
verified
E

At 1 atm pressure,the heat of sublimation of gallium is 277.0kJ/mol and the heat of vaporization is 271.0 kJ/mol.To the correct number of significant figures,how much heat is required to melt 5.50 mol of gallium at 1 atm pressure?

Correct Answer
verified
B

Correct Answer
verified

Use the ΔH°_f and ΔH°_rxninformation provided to calculate ΔH°_f for SO₃(g) ΔH°_{f (kJ/mol)} 2 SO₂(g) + O₂(g) → 2 SO₃(g) ΔH°_rxn= -198 kJ SO₂(g) -297

Correct Answer
verified

Which of the following processes is endothermic?

Correct Answer
verified

Use the ΔH°_f and ΔH°_rxn information provided to calculate ΔH°_f for IF ΔH°_{f (kJ/mol)} IF₇(g) + I₂(g) → IF₅(g) + 2 IF(g) ΔH°_rxn= -89 kJ IF₇(g) 941 IF₅(g) 840

Correct Answer
verified

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/ml by 7.80°C? (The specific heat of the solution is 3.74 J/g∙K.)

Correct Answer
verified

Exam 10: Thermochemistry

It takes 18.2 kJ of energy to raise the temperature of 55.2g of an unknown liquid from 30.0°C to 47.0°C.What is the specific heat of the unknown liquid

Correct AnswerverifiedD

Energy that is associated with the relative positions of electrons and nuclei in atoms and molecules is called

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Which one of the following elements is NOT in its standard state?

Correct AnswerverifiedShow Answer

Which of the following processes are endothermic?

Correct AnswerverifiedShow Answer

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.

Correct AnswerverifiedShow Answer

If a block of gold requires 1.42 kJ of energy to raise the temperature from 120.0°C to 240.0°C,what is the mass of the block? The specific heat capacity of gold is 0.129 J/g-K.

Correct AnswerverifiedShow Answer

Use the bond energies provided to estimate ΔH°rxn for the reaction below. CH3OH(l) + 2 O2(g) → CO2(g) + 2 H2O(g) ΔH°rxn = ? Bond Bond Energy (kJ/mol) C-H 414 C-O 360 C=O 799 O=O 498 O-H 464

Correct AnswerverifiedShow Answer

Give the units of heat capacity.

Correct AnswerverifiedShow Answer

Choose the reaction that illustrates ΔH°f for Mg(NO3) 2.

Correct AnswerverifiedShow Answer

Where does the energy absorbed during an endothermic reaction go?

Correct AnswerverifiedDuring an endothermic reaction,the produ...View AnswerShow Answer

When 10.00 moles of H2(g) reacts with 5.000 mol of O2(g) to form 10.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm.If 683.0 kJ of heat are released during this reaction,and PΔV is equal to -37.00 kJ,then

Correct AnswerverifiedShow Answer

According to the following thermochemical equation,what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO2. SiO2(s) + 4 HF(g) → SiF4(g) + 2 H2O(l) ΔH°rxn = -184 kJ

Correct AnswerverifiedShow Answer

Which of the following statements is TRUE?

Correct AnswerverifiedE

At 1 atm pressure,the heat of sublimation of gallium is 277.0kJ/mol and the heat of vaporization is 271.0 kJ/mol.To the correct number of significant figures,how much heat is required to melt 5.50 mol of gallium at 1 atm pressure?

Correct AnswerverifiedB

Correct AnswerverifiedShow Answer

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g) ΔH°f (kJ/mol) 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJ SO2(g) -297

Correct AnswerverifiedShow Answer

Which of the following processes is endothermic?

Correct AnswerverifiedShow Answer

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF ΔH°f (kJ/mol) IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ IF7(g) 941 IF5(g) 840

Correct AnswerverifiedShow Answer

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/ml by 7.80°C? (The specific heat of the solution is 3.74 J/g∙K.)

Correct AnswerverifiedShow Answer

Correct Answer
verified
D

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. CH₃OH(l) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) ΔH°_rxn= ? Bond Bond Energy (kJ/mol) C-H 414 C-O 360 C=O 799 O=O 498 O-H 464

Correct Answer
verified

Correct Answer
verified

Choose the reaction that illustrates ΔH°_f for Mg(NO₃) ₂.

Correct Answer
verified

Correct Answer
verified
During an endothermic reaction,the produ...
View Answer

When 10.00 moles of H₂(g) reacts with 5.000 mol of O₂(g) to form 10.00 mol of H₂O(l) at 25°C and a constant pressure of 1.00 atm.If 683.0 kJ of heat are released during this reaction,and PΔV is equal to -37.00 kJ,then

Correct Answer
verified

According to the following thermochemical equation,what mass of HF (in g) must react in order to produce 345 kJ of energy? Assume excess SiO₂. SiO₂(s) + 4 HF(g) → SiF₄(g) + 2 H₂O(l) ΔH°_rxn= -184 kJ

Correct Answer
verified

Correct Answer
verified
E

Correct Answer
verified
B

Correct Answer
verified

Use the ΔH°_f and ΔH°_rxninformation provided to calculate ΔH°_f for SO₃(g) ΔH°_{f (kJ/mol)} 2 SO₂(g) + O₂(g) → 2 SO₃(g) ΔH°_rxn= -198 kJ SO₂(g) -297

Correct Answer
verified

Correct Answer
verified

Use the ΔH°_f and ΔH°_rxn information provided to calculate ΔH°_f for IF ΔH°_{f (kJ/mol)} IF₇(g) + I₂(g) → IF₅(g) + 2 IF(g) ΔH°_rxn= -89 kJ IF₇(g) 941 IF₅(g) 840

Correct Answer
verified

Correct Answer
verified