EASY
MYP:4-5
IMPORTANT
Earn 100

Industrial reaction conditions for the production of ammonia is as shown below in the graph:

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Explain with reference to the position of the equilibrium why increasing the pressure of this closed system favours the forward reaction. 

Important Questions on Balance

EASY
MYP:4-5
IMPORTANT
How do you test for the presence of ammonia gas?
EASY
MYP:4-5
IMPORTANT
What do you observe when the test tube of ammonium chloride is heated?
EASY
MYP:4-5
IMPORTANT
When the test tube of ammonium chloride is heated, a white solid is observed at the top of the test tube. Can you identify the substance?
EASY
MYP:4-5
IMPORTANT
When the test tube of ammonium chloride is heated, a white solid is observed at the top of the test tube. Explain why this solid has reformed away from the source of heat?
EASY
MYP:4-5
IMPORTANT

The Haber's process describes the industrial production of ammonia gas on a large scale: N2g+3H2g            2NH3g; H°=-92 kJ mol-1. Predict the effect of the following change on the position of the equilibrium in the process.

Nitrogen gas is added to the system at equilibrium. 

 

EASY
MYP:4-5
IMPORTANT

The Haber's process describes the industrial production of ammonia gas on a large scale: N2g+3H2g            2NH3g; H°=-92 kJ mol-1. Predict the effect of the following change on the position of the equilibrium in the process.

Hydrogen gas is removed from the system at equilibrium. 

 

EASY
MYP:4-5
IMPORTANT

The Haber's process describes the industrial production of ammonia gas on a large scale: N2g+3H2g            2NH3g; H°=-92 kJ mol-1. Predict the effect of the following change on the position of the equilibrium in the process.

The pressure of the system is decreased.

 

EASY
MYP:4-5
IMPORTANT

The Haber's process describes the industrial production of ammonia gas on a large scale: N2g+3H2g            2NH3g; H°=-92 kJ mol-1. Predict the effect of the following change on the position of the equilibrium in the process.

The temperature of the system is increased.