Kinetics and Equilibrium Review

Rate of Reaction

100

What happens to the rate of reaction when a catalyst is added?

Speeds up the rate of reaction

200

What type of compound reacts the fastest as an aqueous solution: Ionic or Covalent?

Ionic

300

In terms of collisions, explain how increasing the concentration increases the rate of reaction.

If the number of particles increases the number of collisions will increase which increases the rate of reaction. 

400

In terms of collisions, explain how decreasing the temperature of a reaction will slow down the rate of reaction. 

Decreasing the temperature decreases the speed at which the particles are moving therefore there are less collisions. 

500

Explain how changing pressure will change the rate of reaction for the following equation:

H₂(g) + I₂(g) --> 2HI(g)

Increasing pressure will increase the rate of reaction by creating more collisions. 

Decreasing pressure will decrease the rate of reaction by creating less collisions. 

Potential Energy Diagrams

100

Using the potential energy diagram on the board, identify the number of the line/point that indicates the potential energy of the reactants

Line 1

200

Using the potential energy diagram on the board, identify the number of the line/point that indicates the heat of reaction

line 6

300

Using the potential energy diagram on the board, identify the number of the line/point that indicates the activated complex

Point 7

400

Using the potential energy diagram on the board, identify the number of the line/point that indicates the activation energy of the reverse reaction

Line 5

500

Using the potential energy diagram on the board, identify all of the numbers of the lines/point that will change when a catalyst is added.

Lines 4, 5, 6, and 7

Le Chatelier's Principal

100

N₂(g) +3H₂(g) --> 2NH₃(g) + heat

Using the reaction above, state the shift in equilibrium when more H₂(g) is added.

Shift right 

200

N₂(g) +3H₂(g) --> 2NH₃(g) + heat

Using the reaction above, state the shift in equilibrium when a catalyst is added.  

no shift

300

N₂(g) +3H₂(g) --> 2NH₃(g) + heat

Using the reaction above, state the shift in equilibrium when temperature is increased

Shift left

400

2HCl(aq) + Mg(s) --> MgCl₂(aq) + H₂(g) + heat

Using the reaction above, state the shift in equilibrium when additional magnesium is added.

No change. 

500

2HCl(aq) + Mg(s) --> MgCl₂(aq) + H₂(g) + heat

Using the reaction above, state the shift in equilibrium when H₂(g) is removed

shift right

Entropy and Enthalpy

100

Is heat located in the reactants or products in an endothermic reaction?

Reactants

200

Does nature favor an increase or decrease in entropy?

Increase in entropy

300

What is the overall change in entropy of the given reaction?

NaCl(s) --> Na⁺(aq) + Cl^-(aq)

increase in entropy

400

Does nature favor an increase or decrease in enthalpy?

Decrease in enthalpy (exothermic)

500

What is the overall change in entropy of the given reaction?

N₂(g) +3H₂(g) --> 2NH₃(g)

Decrease in entropy

Random

100

An effective collision requires ____________ orientation and ___________ energy.

proper orientation and sufficient energy

200

Using the potential energy diagram on the board, identify the number of the line/point that indicates the potential energy of the activated complex

Line 2

300

What two values are subtracted to obtain the heat of reaction?

You may either state their names or reference the numbers on the potential energy diagram on the board

The PE of the products - the PE of the reactants.

lines 3-1

400

What condition(s) are required for a solution to reach equilibrium?

Saturated solution 

500

N₂(g) +3H₂(g) --> 2NH₃(g) + heat

Using the reaction above, state the shift in equilibrium when pressure is decreased

Shift left, to side with more moles of gas.