In the gaseous equilibrium $H_2X_2 + \text{heat} \rightleftharpoons 2HX$,the formation of $HX$ will be favoured by

In which of the following equilibrium reactions does the equilibrium shift to the right when the total pressure is decreased?

In the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$,greater product will be obtained or the forward reaction is favoured by:

Consider the following reaction:
$N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)} ; \Delta H^{0} = +58 \ kJ$
For each of the following cases $(a, b)$,determine the direction in which the equilibrium shifts:
$(a)$ Temperature is decreased
$(b)$ Pressure is increased by adding $N_{2}$ at constant $T$ and constant $V$

The supply of oxygen to tissues by blood can be explained by:

Assertion : $A$ catalyst does not alter the equilibrium constant of a reaction.
Reason : The catalyst forms a complex with the reactants and provides an alternate path with lower energy of activation for the reaction; the forward and the backward reactions are affected to the same extent.