Physical Chemistry Answers

For the reaction system N2(g) + 3H2(g) ⇌ 2NH3(g) at equilibrium, ΔH is -92 kJ. In order to both shift the equilibrium and increase the yield of ammonia, we should

1. increase the temperature

2. decrease the temperature

3. increase the pressure

4. decrease the pressure


A) 1 only
B) 2 only
C) 1 and 3 only
D) 2 and 3 only
E) 1 and 4 only

For the following reaction system at equilibrium, which one of the changes would cause the equilibrium to shift to the right?

2NOBr(g) ⇌ 2NO(g) + Br2(g) ΔHo = 30 kJ


A) Decrease the volume of the reaction vessel.
B) Add some NO.
C) Remove some NOBr.
D) Add Br2.
E) Increase the temperature.

Briefly give various experimental methods for studying the reaction rates

Briefly explain the laws of osmotic pressure

Derive the expression relating equilibrium constant with temparature

Derive the integrated form of clausius-clapeyron equation

For the reaction system 2NH3(g) ⇌ N2(g) + 3H2(g) at equilibrium, ΔH is 92 kJ. In order to increase the value of K for this reaction, we would

1. increase the temperature

2. decrease the temperature

3. increase the pressure

4. decrease the pressure

A) 1 only
B) 2 only
C) 1 and 3 only
D) 2 and 3 only
E) 2 and 4 only

The reaction below is exothermic:
2SO2 (g) + O2 (g) ⇌ 2SO3 (g)

Le Chatelier's Principle predicts that ________ will result in an increase in the number of moles of SO3 (g) in the reaction container.

A) removing some oxygen
B) increasing the temperature
C) decreasing the pressure
D) increasing the pressure
E) increasing the volume of the container

the active mass of 7.0 g of nitrogen in a 2 L container would be