For the equilibrium $C_{(diamond)} \rightleftharpoons C_{(graphite)}$,the densities of diamond and graphite are $3.5 \ g/mL$ and $2.3 \ g/mL$ respectively. What happens to the equilibrium upon increasing the pressure?

For which of the following reactions will a change in the volume of the system $NOT$ result in a change in the number of moles of the components?

Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per the following endothermic reaction:
$CH_{4(g)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + 3H_{2(g)}$
$(a)$ Write an expression for $K_p$ for the above reaction.
$(b)$ How will the values of $K_p$ and the composition of the equilibrium mixture be affected by:
$(i)$ increasing the pressure
$(ii)$ increasing the temperature
$(iii)$ using a catalyst?

Which of the following changes will shift the reaction towards the product?
$I_{2(g)} \rightleftharpoons 2I_{(g)}$ $\Delta H_r^o(298 \ K) = +150 \ kJ$

For a reaction,if $K_p > K_c$,then the forward reaction is favored by ..... $(T > 15 \ K)$

For the reaction: $A + B + Q \rightleftharpoons C + D$,if the temperature is increased,then the concentration of the products will