Kinetics and Equilibrium Review

Given the reaction

S(s) + O₂(g) --> SO₂(g) + energy

Which diagram best represents the potential energy changes for this reaction?

• a

• b

• c

• d

The potential energy diagram below represents a reaction.

Which arrow represents the activation energy of the forward reaction

• A

• B

• C

• D

Given the potential energy diagram for the chemical reaction:

Which statement correctly describes the energy changes that occur in the forward reaction

• The activation energy is 50kJ and the reaction is exothermic

• The activation energy is 50kJ and the reaction is endothermic

• The activation energy is 10kJ and the reaction is exothermic

• The activation energy is 10kJ and the reaction is endothermic

Increasing the temperature increases the rate of a reaction by

• lowering the activation energy

• increasing the frequency of effective collisions between reacting molecules

• lowering the frequency of effective collisions between reacting molecules

• increasing the activation energy

The beakers shown below, a 2.0 centimeter strip of magnesium ribbon reacts with 100 milliliters of HCl(aq) under the conditions shown

In which beaker will the reaction occur at the fastest rate?

• A

• B

• C

• D

At STP, which 4.0-gram zinc sample will react fastest with dilute hydrochloric acid?

• sheet metal

• powdered

• bar

• granules

Grinding a seltzer tablet into powder increases the rate of reaction due to...

• increased concentration of reactants
• increased surface area
• increased speed of particles.
• better orientation of reactants

What is the activation energy?

• The energy of the products
• The energy of the reactants
• The minimum energy needed by the reactants to form the products.
• The energy lost in the reaction

When K_eq > 1, 

• There are more products than reactants when the reaction reached equilibrium.
• There are more reactant than products when the reaction reached equilibrium.
• The amount of reactants is equal to the amount of products.

Define chemical equilibrium.

• A reaction is reversible.
• The concentration of the reactants is equal to the concentration of the products.
• The rate of a forward reaction is equal to the rate of the reverse reaction.
• The reaction stops and no further change in concentration occurs.