In a reversible reaction,a catalyst:

Sodium sulphate dissolves in water with the evolution of heat. Consider a saturated solution of sodium sulphate. If the temperature is raised,then according to Le Chatelier's principle:

The standard state Gibbs free energy change for the given isomerization reaction $cis-2-pentene \rightleftharpoons trans-2-pentene$ is $-3.67 \ kJ/mol$ at $400 \ K$. If more $trans-2-pentene$ is added to the reaction vessel,then:

Which among the following reactions is favoured in the forward direction by an increase in temperature?

For the equilibrium $2NO_{2(g)} \rightleftharpoons N_2O_{4(g)} + 14.6 \ kcal$,the increase in temperature would

The endothermic reaction $(M + N \rightleftharpoons P)$ is allowed to attain an equilibrium at $25^o C$. Formation of $P$ can be increased by