Question

When $NaN{O}_3$ is heated in a closed vessel, oxygen is liberated and $NaN{O}_2$ is left behind. Then at equilibrium:

• A. addition of $NaN{O}_2$ favours reverse reaction
• B. addition of $NaN{O}_2$ favours forward reaction
• C. increasing temperature favours forward reaction
• D. decreasing pressure favours reverse reaction

Answer 1

Answer: (A), (C)

The correct options are
A addition of $NaN{O}_2$ favours reverse reaction
C increasing temperature favours forward reaction

According to Le Chatlier's principle:

Increasing the concentration of product will shift the equilibrium backward, thus the addition of $NaN{O}_2$ favours the reverse direction.

Increasing temperature favours the forward reaction as this is the endothermic direction.

$2NaN{O}_3\left(s\right)\rightleftharpoons 2NaN{O}_2\left(s\right)+O_2\left(g\right)$ (endothermic)

Also, decreasing pressure favours forward reaction.