$A$ reversible reaction is in equilibrium. If a factor is changed which affects it,then:

According to Le Chatelier's principle,adding heat to a solid and liquid in equilibrium with an endothermic nature will cause the:

Consider the equilibrium $CO_{(g)} + 3H_{2(g)} \rightleftharpoons CH_{4(g)} + H_2O_{(g)}$. If the pressure applied over the system increases by two-fold at constant temperature,then which of the following statements are correct?
$(A)$ Concentration of reactants and products increases.
$(B)$ Equilibrium will shift in the forward direction.
$(C)$ Equilibrium constant increases since the concentration of products increases.
$(D)$ Equilibrium constant remains unchanged as the concentration of reactants and products remain the same.
Choose the correct answer from the options given below:

Consider the following reversible reaction at equilibrium,$2H_2O_{(g)} \rightleftharpoons 2H_{2(g)} + O_{2(g)}$; $\Delta H = 241.7 \ kJ$. Which one of the following changes in conditions will lead to maximum decomposition of $H_2O_{(g)}$?

In which of the following reactions,increase in the volume at constant temperature does not affect the number of moles at equilibrium?

Which of the following conditions is favourable for the production of ammonia by Haber's process?