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

In the $N_2 + 3H_2 \rightleftharpoons 2NH_3$ reversible reaction,an increase in pressure will favour:

In a reversible reaction at $300 \ K$,$K_c > K_p$ and $\Delta H = +40 \ kcal$. The product will be obtained in a higher amount on:

In what manner will an increase of pressure affect the following equilibrium equation?
$C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$

Consider the following reaction and determine which of the conditions will shift the equilibrium position to the right?
$4NH_{3(g)} + 5O_{2(g)} \rightleftharpoons 4NO_{(g)} + 6H_2O_{(g)} + \text{Heat}$

When a vapor is heated slowly from $25\,^oC$ at atmospheric pressure,its color initially deepens. When the temperature is increased above $160\,^oC$,the color fades. At $600\,^oC$,the vapor becomes almost colorless,but when the pressure is increased at this temperature,the color deepens again. What is this vapor?