Question 1

Which of the following best describes an oxidation-reduction (redox) reaction?

Accepted Answer

A reaction in which electrons are transferred from one species to another.

Question 2

Which species is being reduced in the following reaction? $$ \mathrm{Cl}_2 + 2\mathrm{Br}^- \rightarrow 2\mathrm{Cl}^- + \mathrm{Br}_2 $$

Accepted Answer

$$ \mathrm{Cl}_2 $$

Question 3

A sample of gas occupies $$ 4.00 \ \mathrm{L}  at$$ $$ 1.00 \ \mathrm{atm} $$ and $$ 300 \ \mathrm{K} . $$What will be its volume at $$ 2.00 \ \mathrm{atm} $$ and $$ 300 \ \mathrm{K} $$, assuming ideal gas behavior?

Accepted Answer

$$ 2.00 \ \mathrm{L} $$

Question 4

Which of the following statements about the First Law of Thermodynamics is correct?

Accepted Answer

The change in internal energy of a system equals the heat added to the system plus the work done on the system.

Question 5

A balloon is filled with $$ 2.00 \ \mathrm{mol}  of $$helium gas at STP ($$ 1.00 \ \mathrm{atm} $$, $$ 273 \ \mathrm{K} ). $$What is the volume of the balloon?

Accepted Answer

$$ 44.8 \ \mathrm{L} $$

Question 6

Which of the following is NOT a state function?

Accepted Answer

Work ($$ w )$$

Question 7

A chemical reaction in a bomb calorimeter releases $$ 500 \ \mathrm{J}  of $$heat. What is the value of $$ \Delta E $$ for the reaction?

Accepted Answer

$$ -500 \ \mathrm{J} $$

Question 8

Which of the following best describes Graham’s Law of Effusion?

Accepted Answer

The rate of effusion of a gas is inversely proportional to the square root of its molar mass.

Question 9

If $$ 2.00 \ \mathrm{g}  of $$hydrogen gas ($$ \mathrm{H}_2 ) $$and $$ 32.0 \ \mathrm{g}  of $$oxygen gas ($$ \mathrm{O}_2 ) $$are mixed in a $$ 10.0 \ \mathrm{L} $$ container at $$ 273 \ \mathrm{K} $$, what is the mole fraction of hydrogen in the mixture?

Accepted Answer

$$ 0.33 $$

Question 10

Which of the following is the correct expression for the ideal gas law?

Accepted Answer

$$ PV = nRT $$

Question 11

A $$ 50.0 \ \mathrm{g} $$ sample of water is heated from $$ 25.0^\circ \mathrm{C}  to$$ $$ 75.0^\circ \mathrm{C} . If $$the specific heat of water is $$ 4.18 \ \mathrm{J} / (\mathrm{g} \cdot ^\circ \mathrm{C}) $$, how much heat is absorbed?

Accepted Answer

$$ 10,450 \ \mathrm{J} $$

Question 12

Which of the following statements about exothermic reactions is true?

Accepted Answer

The enthalpy change ($$ \Delta H ) is $$negative.

Question 13

A gas sample has a pressure of $$ 2.00 \ \mathrm{atm}  in a$$ $$ 5.00 \ \mathrm{L} $$ container at $$ 300 \ \mathrm{K} . $$How many moles of gas are present? ($$ R = 0.0821 \ \mathrm{L} \cdot \mathrm{atm} / \mathrm{mol} \cdot \mathrm{K} )$$

Accepted Answer

$$ 0.41 \ \mathrm{mol} $$

Question 14

Which of the following is a correct application of Dalton’s Law of Partial Pressures?

Accepted Answer

The total pressure of a gas mixture is the sum of the partial pressures of each component gas.

Question 15

Which of the following best describes the relationship between temperature and kinetic energy for an ideal gas?

Accepted Answer

The average kinetic energy of gas particles increases as temperature increases.

Question 16

A $$ 1.00 \ \mathrm{mol} $$ sample of an ideal gas is compressed isothermally from $$ 10.0 \ \mathrm{L}  to$$ $$ 2.00 \ \mathrm{L}  at$$ $$ 300 \ \mathrm{K} . $$What is the change in internal energy ($$ \Delta U ) of $$the gas?

Accepted Answer

$$ 0 \ \mathrm{J} $$

Question 17

Which of the following is the correct formula for calculating heat ($$ q ) $$absorbed or released by a substance?

Accepted Answer

$$ q = m c \Delta T $$

Question 18

Which of the following is a correct statement of Boyle’s Law?

Accepted Answer

At constant temperature, the pressure and volume of a gas are inversely proportional.

Question 19

A reaction has $$ \Delta H = -250 \ \mathrm{kJ} $$ and $$ \Delta S = -100 \ \mathrm{J} / \mathrm{K} . At $$what temperature (in K) does the reaction become non-spontaneous? ($$ \Delta G = \Delta H - T \Delta S )$$

Accepted Answer

$$ 2500 \ \mathrm{K} $$

General Chemistry Exam Study Guide: Thermodynamics, Gas Laws, and Chemical Reactions

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