Q: Which of the following best describes the relationship between $K_c$ and $K_p$ for a gaseous reaction?

$K_p = K_c \times (RT)^{\Delta n}$, where $\Delta n$ is the change in moles of gas

Question 1

Which of the following statements best describes the difference between a state function and an extensive property?

Accepted Answer

A state function is independent of the path taken and depends only on the current state, while an extensive property depends on the amount of substance present.

Question 2

A buffer is made by dissolving 0.12 mol of sodium propionate (NaC2H5COO) in 1.00 L solution that contains 0.09 mol of propionic acid (C2H5COOH). For propionic acid, $K_a = 1.3 	imes 10^{-5}$. What is the pH of the buffer?

Accepted Answer

$pH = 4.87$

Question 3

Which of the following is the correct formula for the hypobromite ion?

Accepted Answer

$BrO^-$

Question 4

Given the reaction $2 CH_4 (g) + 2 H_2O (g) \rightarrow 2 CH_3OH (g) + H_2 (g)$ and the following standard enthalpies of formation: $\Delta H_f^{\circ}(CH_4) = -80.8$ kJ/mol, $\Delta H_f^{\circ}(CH_3OH) = -201.0$ kJ/mol, $\Delta H_f^{\circ}(H_2O) = -241.8$ kJ/mol, what is the standard enthalpy change $\Delta H^{\circ}$ for the reaction?

Accepted Answer

$\Delta H^{\circ} = +80.2$ kJ

Question 5

Which of the following best describes the relationship between $K_c$ and $K_p$ for a gaseous reaction?

Accepted Answer

$K_p = K_c 	imes (RT)^{\Delta n}$, where $\Delta n$ is the change in moles of gas

Question 6

A solution contains 0.0020 M NaOH. What is the pH of the solution?

Accepted Answer

$pH = 11.60$

Question 7

Which of the following is a strong electrolyte?

Accepted Answer

Sodium chloride ($NaCl$)

Question 8

A 1.4 	imes 10^{-3} mol sample of argon is placed in a 250 mL bulb at 27°C. What is the pressure of the argon gas in the bulb? (Use $R = 0.0821$ L·atm·mol$^{-1}$·K$^{-1}$)

Accepted Answer

$P = 0.16$ atm

Question 9

Which of the following best explains why work is considered a path function?

Accepted Answer

Work depends on the specific process or path taken between two states.

Question 10

Which of the following ions has 18 electrons?

Accepted Answer

$Ca^{2+}$

Question 11

Calculate the $pOH$ of a 0.0350 M $Ca(OH)_2$ solution.

Accepted Answer

$pOH = 1.46$

Question 12

Which of the following is true about the equilibrium constant $K_{eq}$ for a reaction?

Accepted Answer

$K_{eq}$ changes with temperature.

Question 13

A solution of 0.1075 M $HNO_3$ is prepared. What is the pH of the solution?

Accepted Answer

$pH = 1.97$

Question 14

Which of the following best describes a weak electrolyte?

Accepted Answer

A substance that partially dissociates into ions in solution.

Question 15

Which of the following is the correct balanced equation for the reaction between cyclohexane ($C_6H_{12}$) and $O_2$ to produce adipic acid ($H_2C_6H_8O_4$) and water?

Accepted Answer

$2 C_6H_{12} + 5 O_2 \rightarrow 2 H_2C_6H_8O_4 + 2 H_2O$

Question 16

Which of the following is the correct expression for the Gibbs free energy change ($\Delta G$) at non-standard conditions?

Accepted Answer

$\Delta G = \Delta G^{\circ} + RT \ln Q$

Question 17

A serving of chicken noodle soup contains 2.5 g fat, 14 g carbohydrates, and 7.0 g protein. What is the total Calorie content of the serving? (Use: Protein and carbohydrates generate 17 kJ/g, fat produces 38 kJ/g. 1 Calorie = 4.184 kJ)

Accepted Answer

Total Calories = 110

Question 18

Which of the following is the correct formula for calculating the equilibrium constant $K_{eq}$ from standard Gibbs free energy change $\Delta G^{\circ}$?

Accepted Answer

$\Delta G^{\circ} = -RT \ln K_{eq}$

Question 19

Which of the following is true about the effect of temperature on the spontaneity of a reaction?

Accepted Answer

A reaction with $\Delta H > 0$ and $\Delta S > 0$ becomes spontaneous at high temperatures.

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