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GRE Subject Test: Chemistry : Reaction Chemistry

Study concepts, example questions & explanations for GRE Subject Test: Chemistry

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Example Questions

Example Question #2 : Reaction Equilibrium

Based on the equilibrium reaction shown, how would adding $H_{2}$ to the system affect the equilibrium?

Possible Answers:

Adding $H_{2}$ to the system would cause the equilibrium to shift to the right, producing more $N_{2}$ in order to reduce the concentration of $NH_{3}$

The effect of adding $H_{2}$ to the system cannot be predicted

Adding $H_{2}$ to the system would cause the equilibrium to shift to the left, producing more $N_{2}$ in order to reduce the concentration of $H_{2}$

Adding $H_{2}$ would not have any effect on the equilibrium

Adding $H_{2}$ to the system would cause the equilibrium to shift to the right, producing more $NH_{3}$ in order to reduce the concentration of $H_{2}$

Correct answer:

Adding $H_{2}$ to the system would cause the equilibrium to shift to the right, producing more $NH_{3}$ in order to reduce the concentration of $H_{2}$

Explanation:

According to Le Chatelier's principle, if an equilibrium reaction is disturbed by addition of a reactant or product, the equilibrium will shift to counteract the disturbance. Therefore, adding $H_{2}$ to the system would cause the equilibrium to shift to the right, producing more $NH_{3}$ in order to reduce the concentration of $H_{2}$ .

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Example Question #2 : Reaction Equilibrium

Which method can be used to decrease the activation energy of a reaction?

Possible Answers:

All of these

Increasing the pressure

Increasing the concentration of reactants

Increasing the temperature

Adding a catalyst

Correct answer:

All of these

Explanation:

The activation energy is the minimum amount of energy required to start a chemical reaction. Based on the collision model, increasing the temperature, pressure, and concentration for a chemical reaction will decrease the activation energy. This is because increasing these factors increases the number of collisions of molecules. Molecules must collide to react.

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Example Question #21 : Solubility And Ions

Which of the following is true regarding the solubility product constant, $\small K_{sp}$ , for a reaction in the form:

$aA_{(s)}\rightleftharpoons cC_{(aq)}+dD_{(aq)}$

Possible Answers:

$\small K_{sp}$ represents the ratio of reactants to products as the reaction progresses

As more of substance $\small A$ dissolves in the given solution, $\small K_{sp}$ increases

$\small K_{sp}$ has units of moles per liter

$K_{sp}=[C]^c[D]^d$

The concentration of substance $\small A$ strongly influences the value of $\small K_{sp}$

Correct answer:

$K_{sp}=[C]^c[D]^d$

Explanation:

To determine the solubility product constant, we only need the concentrations and coefficients of the ions. The effective concentration of any pure substance (solid, liquid, or gas) is equal to one by definition, so does not influence the value of $\small K_{sp}$ . The equation for the solubility product constant of this reaction is:

$K_{sp}=[C]^c[D]^d$

The units of the solubility product constant will depend on the coefficients of the products. $\small K_{sp}$ will be a constant for the reaction, and will not change as more solid dissolves or as the reaction progresses.

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GRE Subject Test: Chemistry : Reaction Chemistry

Study concepts, example questions & explanations for GRE Subject Test: Chemistry

All GRE Subject Test: Chemistry Resources

Example Questions

Example Question #2 : Reaction Equilibrium

Example Question #2 : Reaction Equilibrium

Example Question #21 : Solubility And Ions

All GRE Subject Test: Chemistry Resources

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