Question

In lime kiln, the reversible reaction,

$CaC{O}_3\left(s\right)\rightleftharpoons CaO\left(s\right)+C{O}_2\left(g\right)$

It proceeds to completion because :

• A. of high temperature
• B. $C{O}_2$ escapes out
• C. $CaO$ is removed
• D. of low temperature

Answer 1

The correct option is B $C{O}_2$ escapes out

Removal of the gaseous product always favours forward reaction. The equilibria that involve gases - that is, those equilibria that have different numbers of gaseous molecules on the left and right sides of the equilibrium equation.

Increased pressure favours the reaction that decreases the number of gaseous molecules. Increased pressure decreases the volume available to this gaseous equilibrium and favours the forward reaction.

Hence, option B is correct.