Question 1

The standard temperature is _____; the standard concentration of a solution is _______; and the standard pressure is _____.

Accepted Answer

usually 25

Question 2

Suppose a sample of gas undergoes the following change of state.   Which statement(s)is/are true concerning this change of state? i.w must be positive.
Ii)w must be negative.
Iii)q must be positive.
Iv)q must be negative.

Accepted Answer

A) I only 
B) II only 
C) II and III 
D) II and IV 
E) I and III 
A) I only 
B) II only 
C) II and III 
D) II and IV 
E) I and III

Question 3

The statement,"Energy can neither be destroyed nor created," is the _____________.

Accepted Answer

first law

Question 4

For a particular process,28 kJ of heat is absorbed and 15 kJ of work is done on the surroundings.What is ΔU?

Accepted Answer

A) ΔU = +43 kJ 
B) ΔU = -43 kJ 
C) ΔU = -13 kJ 
D) ΔU = +13 kJ 
E) ΔU = +28 kJ 
A) ΔU = +43 kJ 
B) ΔU = -43 kJ 
C) ΔU = -13 kJ 
D) ΔU = +13 kJ 
E) ΔU = +28 kJ

Question 5

A system delivers 222 J of heat to the surroundings while delivering 645 J of work.What is the change in the internal energy,ΔU,of the system?

Accepted Answer

A) -423 J 
B) +423 J 
C) -867 J 
D) +867 J 
E) -222 J 
A) -423 J 
B) +423 J 
C) -867 J 
D) +867 J 
E) -222 J

Question 6

What is ΔH°rxn for the following reaction? 2C8H18(l)+ 17O2(g)→ 16CO(g)+ 18H2O(l)
2C8H18(l)+ 25O2(g)→ 16CO2(g)+ 18H2O(l)
ΔH°rxn = -11020.kJ/mol
2CO(g)+ O2(g)→ 2CO2(g)
ΔH°rxn = -566.0 kJ/mol

Accepted Answer

A) -11020.kJ/mol 
B) +6492 kJ/mol 
C) -1964 kJ/mol 
D) -6492 kJ/mol 
E) -11586 kJ/mol 
A) -11020.kJ/mol 
B) +6492 kJ/mol 
C) -1964 kJ/mol 
D) -6492 kJ/mol 
E) -11586 kJ/mol

Question 7

To which one of the following reactions,occurring at 25oC,does the symbol ΔHof [H2SO4(l)] refer?

Accepted Answer

A) H2(g)+ S(s)+ 2O2(g) H2SO4(l) 
B) H2SO4(l) H2(g)+ S(s)+ 2O2(g) 
C) H2(g)+ S(g)+ 2O2(g) H2SO4(l) 
D) H2SO4(l) 2 H(g)+ S(s)+ 4O(g) 
E) 2H(g)+S(g)+4O(g) H2SO4(l) 
A) H2(g)+ S(s)+ 2O2(g) H2SO4(l) 
B) H2SO4(l) H2(g)+ S(s)+ 2O2(g) 
C) H2(g)+ S(g)+ 2O2(g) H2SO4(l) 
D) H2SO4(l) 2 H(g)+ S(s)+ 4O(g) 
E) 2H(g)+S(g)+4O(g) H2SO4(l)

Question 8

An ideal gas (the system)is contained in a flexible balloon at a pressure of 1 atm and is initially at a temperature of 20.°C.The surrounding air is at the same pressure,but its temperature is 25°C.When the system has equilibrated with its surroundings,both system and surroundings are at 25°C and 1 atm.In changing from the initial to the final state,which one of the following relationships regarding the system is correct?

Accepted Answer

A) ΔU  0 
E) q > 0 
A) ΔU  0 
E) q > 0

Question 9

The sign of w when work is done by the system on the surroundings is _____________.

Accepted Answer

The answer of The sign of w when work is...

Question 10

What is the change in internal energy in joules for a system that releases 154 J of heat and does 125 J of work on its surroundings?

Accepted Answer

A) -29 J 
B) 279 J 
C) 29 J 
D) 1.23 J 
E) -279 J 
A) -29 J 
B) 279 J 
C) 29 J 
D) 1.23 J 
E) -279 J

Question 11

Ozone (O3)in the atmosphere can be converted to oxygen gas by reaction with nitric oxide (NO).(Nitrogen dioxide is also produced in the reaction.)What is the enthalpy change when 8.50 L of ozone at a pressure of 1.00 atm and 25°C reacts with 12.00 L of nitric oxide at the same initial pressure and temperature (R = 0.0821 L atm/mol K)? [ΔH°f(NO)= 90.4 kJ/mol; ΔH°f(NO2)= 33.85 kJ/mol; ΔH°f(O3)= 142.2 kJ/mol]

Accepted Answer

A) -69.1 kJ 
B) -19.7 kJ 
C) -1690 kJ 
D) -97.6 kJ 
E) -167 kJ 
A) -69.1 kJ 
B) -19.7 kJ 
C) -1690 kJ 
D) -97.6 kJ 
E) -167 kJ

Question 12

How many calories are in 854.3 J? (1 cal = 4.184 J)

Accepted Answer

A) 4.897 × 10-3 cal 
B) 204.2 cal 
C) 1.171 ×10-3 cal 
D) 0.2390 cal 
E) 3574 cal 
A) 4.897 × 10-3 cal 
B) 204.2 cal 
C) 1.171 ×10-3 cal 
D) 0.2390 cal 
E) 3574 cal

Question 13

When heat is absorbed by the system and work is done by the system on the surroundings then

Accepted Answer

A) q is negative and w is positive. 
B) both q and w are positive. 
C) both q and w are negative. 
D) q is positive and w is negative. 
E) both q and W are zero. 
A) q is negative and w is positive. 
B) both q and w are positive. 
C) both q and w are negative. 
D) q is positive and w is negative. 
E) both q and W are zero.

Question 14

Which type of system may transfer energy,but not mass,to the surroundings?

Accepted Answer

A) mass transfer system 
B) isolated system 
C) closed system 
D) nonenergy system 
E) open system 
A) mass transfer system 
B) isolated system 
C) closed system 
D) nonenergy system 
E) open system

The standard temperature is _; the standard concentration of a solution is _; and the standard pressure is ___.

Suppose a sample of gas undergoes the following change of state. Which statement(s)is/are true concerning this change of state? i.w must be positive. Ii)w must be negative. Iii)q must be positive. Iv)q must be negative.

The statement,"Energy can neither be destroyed nor created," is the _____________.

For a particular process,28 kJ of heat is absorbed and 15 kJ of work is done on the surroundings.What is ΔU?

A system delivers 222 J of heat to the surroundings while delivering 645 J of work.What is the change in the internal energy,ΔU,of the system?

What is ΔH°_rxn for the following reaction? 2C₈H₁₈(l)+ 17O₂(g)→ 16CO(g)+ 18H₂O(l) 2C₈H₁₈(l)+ 25O₂(g)→ 16CO₂(g)+ 18H₂O(l) ΔH°_rxn = -11020.kJ/mol 2CO(g)+ O₂(g)→ 2CO₂(g) ΔH°_rxn = -566.0 kJ/mol

To which one of the following reactions,occurring at 25^oC,does the symbol ΔH^o_f [H₂SO₄(l)] refer?

The sign of w when work is done by the system on the surroundings is _____________.

What is the change in internal energy in joules for a system that releases 154 J of heat and does 125 J of work on its surroundings?

How many calories are in 854.3 J? (1 cal = 4.184 J)

When heat is absorbed by the system and work is done by the system on the surroundings then

Which type of system may transfer energy,but not mass,to the surroundings?

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

Exam 5: Thermochemistry

The standard temperature is _____; the standard concentration of a solution is _______; and the standard pressure is _____.

Suppose a sample of gas undergoes the following change of state. Which statement(s)is/are true concerning this change of state? i.w must be positive. Ii)w must be negative. Iii)q must be positive. Iv)q must be negative.

The statement,"Energy can neither be destroyed nor created," is the _____________.

For a particular process,28 kJ of heat is absorbed and 15 kJ of work is done on the surroundings.What is ΔU?

A system delivers 222 J of heat to the surroundings while delivering 645 J of work.What is the change in the internal energy,ΔU,of the system?

What is ΔH°rxn for the following reaction? 2C8H18(l)+ 17O2(g)→ 16CO(g)+ 18H2O(l) 2C8H18(l)+ 25O2(g)→ 16CO2(g)+ 18H2O(l) ΔH°rxn = -11020.kJ/mol 2CO(g)+ O2(g)→ 2CO2(g) ΔH°rxn = -566.0 kJ/mol

To which one of the following reactions,occurring at 25oC,does the symbol ΔHof [H2SO4(l)] refer?

The sign of w when work is done by the system on the surroundings is _____________.

What is the change in internal energy in joules for a system that releases 154 J of heat and does 125 J of work on its surroundings?

How many calories are in 854.3 J? (1 cal = 4.184 J)

When heat is absorbed by the system and work is done by the system on the surroundings then

Which type of system may transfer energy,but not mass,to the surroundings?

Chemistry: the Central Science

Atoms Molecules and Ions

Stoichiometry Ratios of Combination

Reactions in Aqueous Solutions

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

Chemical Bonding Ii Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

The standard temperature is _; the standard concentration of a solution is _; and the standard pressure is ___.

What is ΔH°_rxn for the following reaction? 2C₈H₁₈(l)+ 17O₂(g)→ 16CO(g)+ 18H₂O(l) 2C₈H₁₈(l)+ 25O₂(g)→ 16CO₂(g)+ 18H₂O(l) ΔH°_rxn = -11020.kJ/mol 2CO(g)+ O₂(g)→ 2CO₂(g) ΔH°_rxn = -566.0 kJ/mol

To which one of the following reactions,occurring at 25^oC,does the symbol ΔH^o_f [H₂SO₄(l)] refer?