Question 1

In a bomb calorimeter,reactions are carried out

Accepted Answer

A)  at fixed pressure. 
B)  at fixed volume. 
C)  at fixed temperature. 
D)  with solids only. 
E)  using water as a solvent. 
A)  at fixed pressure. 
B)  at fixed volume. 
C)  at fixed temperature. 
D)  with solids only. 
E)  using water as a solvent.

Question 2

According to the following reaction,how much energy is evolved during the reaction of 0.111 mol B2H6 and 0.252 mol Cl2 (Both gases are initially at STP)? 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)  58.7 kJ 
B)  156 kJ 
C)  215 kJ 
D)  352 kJ 
E)  508 kJ 
A)  58.7 kJ 
B)  156 kJ 
C)  215 kJ 
D)  352 kJ 
E)  508 kJ

Question 3

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction P4(g)+ 10 Cl2(g)→ 4PCl5(s)ΔH°rxn = ?
Given:
PCl5(s)→ PCl3(g)+ Cl2(g)ΔH°rxn = +157 kJ
P4(g)+ 6 Cl2(g)→ 4 PCl3(g)ΔH°rxn = -1207 kJ

Accepted Answer

A)  -1835 kJ 
B)  -1364 kJ 
C)  -1050. kJ 
D)  -1786 kJ 
E)  -2100. kJ 
A)  -1835 kJ 
B)  -1364 kJ 
C)  -1050. kJ 
D)  -1786 kJ 
E)  -2100. kJ

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

Given w = 0,an endothermic reaction has the following.

Accepted Answer

A)  +ΔH and -ΔE 
B)  - ΔH and +ΔE 
C)  + ΔH and +ΔE 
D)  - ΔH and -ΔE 
A)  +ΔH and -ΔE 
B)  - ΔH and +ΔE 
C)  + ΔH and +ΔE 
D)  - ΔH and -ΔE

Question 6

Which statement is FALSE?

Accepted Answer

A)  An exothermic reaction gives heat off heat to the surroundings. 
B)  Enthalpy is the sum of a system's internal energy and the product of pressure and volume change. 
C)  ΔErxn is a measure of heat. 
D)  ΔHrxn is the heat of reaction. 
E)  Endothermic has a positive ΔH. 
A)  An exothermic reaction gives heat off heat to the surroundings. 
B)  Enthalpy is the sum of a system's internal energy and the product of pressure and volume change. 
C)  ΔErxn is a measure of heat. 
D)  ΔHrxn is the heat of reaction. 
E)  Endothermic has a positive ΔH.

Question 7

Which compound should have the largest lattice energy?

Accepted Answer

A)  SrI2 
B)  CaCl2 
C)  NaI 
D)  MgO 
E)  KF 
A)  SrI2 
B)  CaCl2 
C)  NaI 
D)  MgO 
E)  KF

Question 8

Define kinetic energy.

Accepted Answer

A)  energy associated with the temperature of an object 
B)  energy associated with the motion of an object 
C)  energy associated with the force of an object 
D)  energy associated with the gravity of an object 
E)  energy associated with the position or composition of an object 
A)  energy associated with the temperature of an object 
B)  energy associated with the motion of an object 
C)  energy associated with the force of an object 
D)  energy associated with the gravity of an object 
E)  energy associated with the position or composition of an object

Question 9

Two solutions,initially at 24.69°C,are mixed in a coffee cup calorimeter (Ccal = 105.5 J/°C).When a 200.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.100 M NaCl solution,the temperature in the calorimeter rises to 25.16°C.Determine the DH°rxn,in units of kJ/mol AgCl.Assume that the density and heat capacity of the solutions is the same as that of water.Hint: Write a balanced reaction for the process.

Accepted Answer

A)  -32 kJ/mol AgCl 
B)  -78 kJ/mol AgCl 
C)  -64 kJ/mol AgCl 
D)  -25 kJ/mol AgCl 
E)  -59 kJ/mol AgCl 
A)  -32 kJ/mol AgCl 
B)  -78 kJ/mol AgCl 
C)  -64 kJ/mol AgCl 
D)  -25 kJ/mol AgCl 
E)  -59 kJ/mol AgCl

Question 10

Use the bond energies provided to estimate ΔH°rxn for the reaction below. XeF2 + 2 F2 → XeF6 ΔH°rxn = ?
Bond Bond Energy (kJ/mol)
Xe-F 147
F-F 159

Accepted Answer

A)  -429 kJ 
B)  +159 kJ 
C)  -660 kJ 
D)  +176 kJ 
E)  -270 kJ 
A)  -429 kJ 
B)  +159 kJ 
C)  -660 kJ 
D)  +176 kJ 
E)  -270 kJ

Question 11

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction:     (l)→   O(l)+   (g)ΔH = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

Accepted Answer

A)  -23.1 kJ 
B)  -11.5 kJ 
C)  -0.0217 kJ 
D)  1.44 kJ 
E)  -2.31 × 104 kJ 
A)  -23.1 kJ 
B)  -11.5 kJ 
C)  -0.0217 kJ 
D)  1.44 kJ 
E)  -2.31 × 104 kJ

Question 12

Which of the following processes is exothermic?

Accepted Answer

A)  a candle flame 
B)  baking bread 
C)  the chemical reaction in a "cold pack" often used to treat injuries 
D)  the vaporization of water 
E)  None of the above are exothermic. 
A)  a candle flame 
B)  baking bread 
C)  the chemical reaction in a "cold pack" often used to treat injuries 
D)  the vaporization of water 
E)  None of the above are exothermic.

Question 13

A sample of copper absorbs 43.6 kJ of heat,resulting in a temperature rise of 75.0°C,determine the mass (in kg)of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.

Accepted Answer

A)  1.51 kg 
B)  6.62 kg 
C)  1.26 kg 
D)  7.94 kg 
E)  3.64 kg 
A)  1.51 kg 
B)  6.62 kg 
C)  1.26 kg 
D)  7.94 kg 
E)  3.64 kg

Question 14

Match between columns
                        Premises: +w
"-w"
-q
+ q
+ΔE

Accepted Answer

The Answer of energy flows into the system from the is...

Question 15

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

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 16

Which of the following processes is endothermic?

Accepted Answer

A)  mixing water and acid 
B)  rusting iron 
C)  photosynthesis 
D)  the electron affinity of a fluorine atom 
E)  None of the above processes are endothermic. 
A)  mixing water and acid 
B)  rusting iron 
C)  photosynthesis 
D)  the electron affinity of a fluorine atom 
E)  None of the above processes are endothermic.

Question 17

Using the following equation for the combustion of octane,calculate the amount of moles of oxygen that reacts with 100.0 g of octane.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

Accepted Answer

A)  18.18 moles 
B)  6.997 moles 
C)  14.00 moles 
D)  8.000 moles 
E)  10.93 moles 
A)  18.18 moles 
B)  6.997 moles 
C)  14.00 moles 
D)  8.000 moles 
E)  10.93 moles

Question 18

A student is preparing to perform a series of calorimetry experiments.She first wishes to determine the calorimeter constant (Ccal)for her coffee cup calorimeter.She pours a 50.0 mL sample of water at 345 K into the calorimeter containing a 50.0 mL sample of water at 298 K.She carefully records the final temperature of the water as 317 K.What is the value of Ccal for the calorimeter?

Accepted Answer

A)  19 J/K 
B)  28 J/K 
C)  99 J/K 
D)  21 J/K 
E)  76 J/K 
A)  19 J/K 
B)  28 J/K 
C)  99 J/K 
D)  21 J/K 
E)  76 J/K

Question 19

A 35.6 g sample of ethanol (C2H5OH)is burned in a bomb calorimeter,according to the following reaction.If the temperature rose from 35.0 to 76.0°C and the heat capacity of the calorimeter is 23.3 kJ/°C,what is the value of DH°rxn? The molar mass of ethanol is 46.07 g/mol.
C2H5OH(l)+ 3 O2(g)→ 2 CO2(g)+ 3 H2O(g)ΔH°rxn = ?

Accepted Answer

A)  -1.24 × 103 kJ/mol 
B)  +1.24 × 103 kJ/mol 
C)  -8.09 × 103 kJ/mol 
D)  -9.55 × 103 kJ/mol 
E)  +9.55 × 103 kJ/mol 
A)  -1.24 × 103 kJ/mol 
B)  +1.24 × 103 kJ/mol 
C)  -8.09 × 103 kJ/mol 
D)  -9.55 × 103 kJ/mol 
E)  +9.55 × 103 kJ/mol

Question 20

The law of ________ states that energy that can be neither created or destroyed.

Accepted Answer

A)  kinetic energy 
B)  the consecration of energy 
C)  potential energy 
D)  the conservation of energy 
E)  thermochemistry 
A)  kinetic energy 
B)  the consecration of energy 
C)  potential energy 
D)  the conservation of energy 
E)  thermochemistry

In a bomb calorimeter,reactions are carried out

According to the following reaction,how much energy is evolved during the reaction of 0.111 mol B₂H₆ and 0.252 mol Cl₂(Both gases are initially at STP)? The molar mass of B₂H₆is 27.67 g/mol. B₂H₆(g)+ 6 Cl₂(g)→ 2 BCl₃(g)+ 6 HCl(g)ΔH°_rxn= -1396 kJ

Use the standard reaction enthalpies given below to determine ΔH°_rxn for the following reaction P₄(g)+ 10 Cl₂(g)→ 4PCl₅(s)ΔH°_rxn= ? Given: PCl₅(s)→ PCl₃(g)+ Cl₂(g)ΔH°_rxn= +157 kJ P₄(g)+ 6 Cl₂(g)→ 4 PCl₃(g)ΔH°_rxn = -1207 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

Given w = 0,an endothermic reaction has the following.

Which statement is FALSE?

Which compound should have the largest lattice energy?

Define kinetic energy.

Use the bond energies provided to estimate ΔH°_rxn for the reaction below. XeF_{2 +}2 F₂ → XeF₆ ΔH°_rxn= ? Bond Bond Energy (kJ/mol) Xe-F 147 F-F 159

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: (l)→ O(l)+ (g)ΔH = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

Which of the following processes is exothermic?

A sample of copper absorbs 43.6 kJ of heat,resulting in a temperature rise of 75.0°C,determine the mass (in kg)of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.

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

Which of the following processes is endothermic?

Using the following equation for the combustion of octane,calculate the amount of moles of oxygen that reacts with 100.0 g of octane.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O ΔH°_rxn= -11018 kJ

The law of ________ states that energy that can be neither created or destroyed.

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

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Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

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Exam 10: Thermochemistry

In a bomb calorimeter,reactions are carried out

According to the following reaction,how much energy is evolved during the reaction of 0.111 mol B2H6 and 0.252 mol Cl2 (Both gases are initially at STP)? 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

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction P4(g)+ 10 Cl2(g)→ 4PCl5(s)ΔH°rxn = ? Given: PCl5(s)→ PCl3(g)+ Cl2(g)ΔH°rxn = +157 kJ P4(g)+ 6 Cl2(g)→ 4 PCl3(g)ΔH°rxn = -1207 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

Given w = 0,an endothermic reaction has the following.

Which statement is FALSE?

Which compound should have the largest lattice energy?

Define kinetic energy.

Use the bond energies provided to estimate ΔH°rxn for the reaction below. XeF2 + 2 F2 → XeF6 ΔH°rxn = ? Bond Bond Energy (kJ/mol) Xe-F 147 F-F 159

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: (l)→ O(l)+ (g)ΔH = -196 kJ Calculate the value of q (kJ)in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?

Which of the following processes is exothermic?

A sample of copper absorbs 43.6 kJ of heat,resulting in a temperature rise of 75.0°C,determine the mass (in kg)of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.

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

Which of the following processes is endothermic?

Using the following equation for the combustion of octane,calculate the amount of moles of oxygen that reacts with 100.0 g of octane.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ

The law of ________ states that energy that can be neither created or destroyed.

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

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According to the following reaction,how much energy is evolved during the reaction of 0.111 mol B₂H₆ and 0.252 mol Cl₂(Both gases are initially at STP)? The molar mass of B₂H₆is 27.67 g/mol. B₂H₆(g)+ 6 Cl₂(g)→ 2 BCl₃(g)+ 6 HCl(g)ΔH°_rxn= -1396 kJ

Use the standard reaction enthalpies given below to determine ΔH°_rxn for the following reaction P₄(g)+ 10 Cl₂(g)→ 4PCl₅(s)ΔH°_rxn= ? Given: PCl₅(s)→ PCl₃(g)+ Cl₂(g)ΔH°_rxn= +157 kJ P₄(g)+ 6 Cl₂(g)→ 4 PCl₃(g)ΔH°_rxn = -1207 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 bond energies provided to estimate ΔH°_rxn for the reaction below. XeF_{2 +}2 F₂ → XeF₆ ΔH°_rxn= ? Bond Bond Energy (kJ/mol) Xe-F 147 F-F 159

Using the following equation for the combustion of octane,calculate the amount of moles of oxygen that reacts with 100.0 g of octane.The molar mass of octane is 114.33 g/mole.The molar mass of carbon dioxide is 44.0095 g/mole. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O ΔH°_rxn= -11018 kJ