In the production of $NO$,the reaction is $N_2(g) + O_2(g) \rightleftharpoons 2NO(g)$,$\Delta H = +ve$. This reaction is favored by:

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,in which direction will the equilibrium shift if an inert gas is added at constant pressure?

Consider the following equation:
$2 SO_{2(g)} + O_{2(g)} \rightleftharpoons 2 SO_{3(g)}, \Delta H = -190 \ kJ$
The number of factors which will increase the yield of $SO_3$ at equilibrium from the following is $.............$.
$A.$ Increasing temperature
$B.$ Increasing pressure
$C.$ Adding more $SO_2$
$D.$ Adding more $O_2$
$E.$ Addition of catalyst

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

The reaction $CaCO_3 \rightleftharpoons CaO + CO_2$ goes to completion in an open vessel because:

The colour of $CrO_4^{2-}(aq.)$ is not changed by: