For an exothermic reaction,the equilibrium constant:

On the basis of the $Le \ Chatelier$ principle,explain how temperature and pressure can be adjusted to increase the yield of ammonia in the following reaction: $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$; $\Delta H = -92.38 \ kJ \ mol^{-1}$. What will be the effect of the addition of argon to the above reaction mixture at constant volume?

The reaction $CaCO_3 \rightleftharpoons CaO + CO_2$ goes to completion in a lime kiln because:

In the reaction ${A_2}_{(g)} + 4{B_2}_{(g)} \rightleftharpoons 2A{B_4}_{(g)}$ where $\Delta H < 0$,the formation of $AB_{4(g)}$ will be favoured by:

For the reaction; $3X_{(g)} + Y_{(g)} \rightleftharpoons X_3Y_{(g)}$,the amount of $X_3Y$ at equilibrium is affected by

Le Chatelier's principle is applicable to: