Question 1

Which of the following has a standard enthalpy of formation value of zero at 25°C?

Accepted Answer

A)  I(g) 
B)  I2(l) 
C)  I2(s) 
D)  I(s) 
E)  I2(g) 
A)  I(g) 
B)  I2(l) 
C)  I2(s) 
D)  I(s) 
E)  I2(g)

Question 2

Which of the following thermodynamic quantities are state functions: heat (q),work (w),enthalpy change ($\Delta$H),and/or internal energy change ($\Delta$U)?

Accepted Answer

A)  q only 
B)  w only 
C)  ($\Delta$H) only 
D)  ($\Delta$U) only 
E)  ($\Delta$H) and ($\Delta$U) 
A)  q only 
B)  w only 
C)  ($\Delta$H) only 
D)  ($\Delta$U) only 
E)  ($\Delta$H) and ($\Delta$U)

Question 3

Which of these physical changes would require the release of energy?

Accepted Answer

A)  condensing a gas 
B)  boiling a liquid 
C)  melting a solid 
D)  all of these 
E)  none of these 
A)  condensing a gas 
B)  boiling a liquid 
C)  melting a solid 
D)  all of these 
E)  none of these

Question 4

Heat capacity is defined as

Accepted Answer

A)  the amount of heat required to raise the temperature of 1 gram of substance by 1 K. 
B)  the amount of heat required to raise the temperature of a substance by 1 K. 
C)  the amount of heat required to vaporize a solid or liquid. 
D)  the maximum amount of heat that a substance may absorb without decomposing. 
E)  4.18 cal/g.K. 
A)  the amount of heat required to raise the temperature of 1 gram of substance by 1 K. 
B)  the amount of heat required to raise the temperature of a substance by 1 K. 
C)  the amount of heat required to vaporize a solid or liquid. 
D)  the maximum amount of heat that a substance may absorb without decomposing. 
E)  4.18 cal/g.K.

Question 5

When 0.236 mol of a weak base (A-)is reacted with excess HCl,6.91 kJ of energy is released as heat.What is $\Delta$H for this reaction per mole of A- consumed?

Accepted Answer

A)  -34.2 kJ/mol 
B)  -59.4 kJ/mol 
C)  -29.3 kJ/mol 
D)  34.2 kJ/mol 
E)  29.3 kJ/mol 
A)  -34.2 kJ/mol 
B)  -59.4 kJ/mol 
C)  -29.3 kJ/mol 
D)  34.2 kJ/mol 
E)  29.3 kJ/mol

Question 6

If 50.0 g of benzene,C6H6,at 25.0 S1U1P1$\circ$S1S1P0C absorbs 2.71 kJ of energy in the form of heat,what is the final temperature of the benzene? The specific heat capacity of benzene is 1.72 J/g.K.

Accepted Answer

A)  25.0 S1U1P1$\circ$S1S1P0C 
B)  31.5 S1U1P1$\circ$S1S1P0C 
C)  56.5 S1U1P1$\circ$S1S1P0C 
D)  32.3 S1U1P1$\circ$S1S1P0C 
E)  57.3 S1U1P1$\circ$S1S1P0C 
A)  25.0 S1U1P1$\circ$S1S1P0C 
B)  31.5 S1U1P1$\circ$S1S1P0C 
C)  56.5 S1U1P1$\circ$S1S1P0C 
D)  32.3 S1U1P1$\circ$S1S1P0C 
E)  57.3 S1U1P1$\circ$S1S1P0C

Question 7

Specific heat capacity is

Accepted Answer

A)  the quantity of heat needed to change the temperature of 1.00 g of a substance by 1 K. 
B)  the quantity of heat needed to change the temperature of 1.00 g of a substance by 4.184 K. 
C)  the capacity of a substance to gain or lose a 1.00 J of energy in the form of heat. 
D)  the temperature change undergone when 1.00 g of a substance absorbs 4.184 J. 
E)  the maximum amount of energy in the form of heat that 1.00 g of a substance may absorb without decomposing. 
A)  the quantity of heat needed to change the temperature of 1.00 g of a substance by 1 K. 
B)  the quantity of heat needed to change the temperature of 1.00 g of a substance by 4.184 K. 
C)  the capacity of a substance to gain or lose a 1.00 J of energy in the form of heat. 
D)  the temperature change undergone when 1.00 g of a substance absorbs 4.184 J. 
E)  the maximum amount of energy in the form of heat that 1.00 g of a substance may absorb without decomposing.

Question 8

When 50.0 mL of 1.30 M of HCl(aq)is combined with 50.0 mL of 1.20 M of NaOH(aq)in a coffee-cup calorimeter,the temperature of the solution increases by 8.01°C.What is the change in enthalpy for this balanced reaction?

HCl(aq)+ NaOH(aq)$\to$ NaCl(aq)+ H2O(l)

Assume that the solution density is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g.S1U1P1$\circ$S1S1P0C.

Accepted Answer

A)  -55.8 kJ 
B)  55.8 kJ 
C)  51.5 kJ 
D)  -51.5 kJ 
E)  -26.8 kJ 
A)  -55.8 kJ 
B)  55.8 kJ 
C)  51.5 kJ 
D)  -51.5 kJ 
E)  -26.8 kJ

Question 9

Using the following thermochemical data:
 
Calculate $\Delta$rHS1U1P1$\circ$S1S1P0 for the following reaction:
HoF3(s)+ 3HCl(g)$\to$ HoCl3(s)+ 3HF(g)

Accepted Answer

A)  -3244.4 kJ/mol-rxn 
B)  330.4 kJ/mol-rxn 
C)  165.2 kJ/mol-rxn 
D)  660.8 kJ/mol-rxn 
E)  -1622.2 kJ/mol-rxn 
A)  -3244.4 kJ/mol-rxn 
B)  330.4 kJ/mol-rxn 
C)  165.2 kJ/mol-rxn 
D)  660.8 kJ/mol-rxn 
E)  -1622.2 kJ/mol-rxn

Question 10

Given the thermochemical equation

Find $\Delta$rHº for the following reaction.

Accepted Answer

A)  (+88.2 kJ/mol-rxn) 
B)  (+264.5  kJ/mol-rxn) 
C)  ( +529.0 kJ/mol-rxn) 
D)  (-176.3 kJ/mol-rxn) 
E)  (-176.3 kJ/mol-rxn). 
A)  (+88.2 kJ/mol-rxn) 
B)  (+264.5  kJ/mol-rxn) 
C)  ( +529.0 kJ/mol-rxn) 
D)  (-176.3 kJ/mol-rxn) 
E)  (-176.3 kJ/mol-rxn).

Question 11

Determine $\Delta$rHS1U1P1$\circ$S1S1P0 for the following reaction,
2 NH3(g)+ 5/2 O2(g)$\to$ 2 NO(g)+ 3 H2O(g)
Given the thermochemical equations below.

Accepted Answer

A)  -1178.2 kJ/mol-rxn 
B)  -452.8 kJ/mol-rxn 
C)  -394.6 kJ/mol-rxn 
D)  -211.0 kJ/mol-rxn 
E)  +1178.2 kJ/mol-rxn 
A)  -1178.2 kJ/mol-rxn 
B)  -452.8 kJ/mol-rxn 
C)  -394.6 kJ/mol-rxn 
D)  -211.0 kJ/mol-rxn 
E)  +1178.2 kJ/mol-rxn

Question 12

Which of the following processes is/are exothermic?
1)the reaction of butane with oxygen
2)the melting of gold
3)cooling copper from 225 S1U1P1$\circ$S1S1P0C to 65 S1U1P1$\circ$S1S1P0C

Accepted Answer

A)  1 only 
B)  2 only 
C)  3 only 
D)  1 and 3 
E)  1,2,and 3 
A)  1 only 
B)  2 only 
C)  3 only 
D)  1 and 3 
E)  1,2,and 3

Question 13

If q = 98 kJ and w = 4 kJ for a certain process,that process

Accepted Answer

A)  requires a catalyst. 
B)  is endothermic. 
C)  occurs slowly. 
D)  is exothermic. 
E)  cannot occur. 
A)  requires a catalyst. 
B)  is endothermic. 
C)  occurs slowly. 
D)  is exothermic. 
E)  cannot occur.

Question 14

Dry ice converts directly from a solid to a gas when heated.This process is called ________.

Accepted Answer

The answer of Dry ice converts directly from a solid...

Which of the following has a standard enthalpy of formation value of zero at 25°C?

Which of the following thermodynamic quantities are state functions: heat (q),work (w),enthalpy change ( $\Delta$ H),and/or internal energy change ( $\Delta$ U)?

Which of these physical changes would require the release of energy?

Heat capacity is defined as

When 0.236 mol of a weak base (A^-)is reacted with excess HCl,6.91 kJ of energy is released as heat.What is $\Delta$ H for this reaction per mole of A^- consumed?

If 50.0 g of benzene,C₆H₆,at 25.0 ^$\circ$C absorbs 2.71 kJ of energy in the form of heat,what is the final temperature of the benzene? The specific heat capacity of benzene is 1.72 J/g.K.

Specific heat capacity is

Given the thermochemical equation $Given the thermochemical equation Find \Delta <sub>r</sub>Hº for the following reaction.$ Find $\Delta$ _rHº for the following reaction. $Given the thermochemical equation Find \Delta <sub>r</sub>Hº for the following reaction.$

Which of the following processes is/are exothermic? 1)the reaction of butane with oxygen 2)the melting of gold 3)cooling copper from 225 ^$\circ$C to 65 ^$\circ$C

If q = 98 kJ and w = 4 kJ for a certain process,that process

Dry ice converts directly from a solid to a gas when heated.This process is called ________.

Basic Concepts of Chemistry

Mathlets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Chemistry of Solids

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Reactivity: Chemical Equilibria

The Chemistry of Acids and Bases

Principles of Reactivity: Other Aspects of Aqueous Equilibria

Entropy and Free Energy

Principles of Reactivity: Electron Transfer Reactions

Environmental Chemistry Earths Environment,energy,and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Exam 6: Principles of Chemical Reactivity: Energy and Chemical Reactions

Which of the following has a standard enthalpy of formation value of zero at 25°C?

Which of the following thermodynamic quantities are state functions: heat (q),work (w),enthalpy change ( Δ\DeltaΔ H),and/or internal energy change ( Δ\DeltaΔ U)?

Which of these physical changes would require the release of energy?

Heat capacity is defined as

When 0.236 mol of a weak base (A-)is reacted with excess HCl,6.91 kJ of energy is released as heat.What is Δ\DeltaΔ H for this reaction per mole of A- consumed?

If 50.0 g of benzene,C6H6,at 25.0 ∘\circ∘ C absorbs 2.71 kJ of energy in the form of heat,what is the final temperature of the benzene? The specific heat capacity of benzene is 1.72 J/g.K.

Specific heat capacity is

Using the following thermochemical data: Calculate Δ\DeltaΔ rH ∘\circ∘ for the following reaction: HoF3(s)+ 3HCl(g) →\to→ HoCl3(s)+ 3HF(g)

Given the thermochemical equation Find Δ\DeltaΔ rHº for the following reaction.

Determine Δ\DeltaΔ rH ∘\circ∘ for the following reaction, 2 NH3(g)+ 5/2 O2(g) →\to→ 2 NO(g)+ 3 H2O(g) Given the thermochemical equations below.

Which of the following processes is/are exothermic? 1)the reaction of butane with oxygen 2)the melting of gold 3)cooling copper from 225 ∘\circ∘ C to 65 ∘\circ∘ C

If q = 98 kJ and w = 4 kJ for a certain process,that process

Dry ice converts directly from a solid to a gas when heated.This process is called ________.

Basic Concepts of Chemistry

Mathlets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Chemistry of Solids

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Reactivity: Chemical Equilibria

The Chemistry of Acids and Bases

Principles of Reactivity: Other Aspects of Aqueous Equilibria

Entropy and Free Energy

Principles of Reactivity: Electron Transfer Reactions

Environmental Chemistry Earths Environment,energy,and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Which of the following thermodynamic quantities are state functions: heat (q),work (w),enthalpy change ( $\Delta$ H),and/or internal energy change ( $\Delta$ U)?

When 0.236 mol of a weak base (A^-)is reacted with excess HCl,6.91 kJ of energy is released as heat.What is $\Delta$ H for this reaction per mole of A^- consumed?

If 50.0 g of benzene,C₆H₆,at 25.0 ^$\circ$C absorbs 2.71 kJ of energy in the form of heat,what is the final temperature of the benzene? The specific heat capacity of benzene is 1.72 J/g.K.

Given the thermochemical equation $Given the thermochemical equation Find \Delta <sub>r</sub>Hº for the following reaction.$ Find $\Delta$ _rHº for the following reaction. $Given the thermochemical equation Find \Delta <sub>r</sub>Hº for the following reaction.$

Which of the following processes is/are exothermic? 1)the reaction of butane with oxygen 2)the melting of gold 3)cooling copper from 225 ^$\circ$C to 65 ^$\circ$C