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

On increasing temperature,the equilibrium constant of exothermic and endothermic reactions,respectively

How will an increase in pressure affect the following equilibrium? $C_{(s)} + H_2O_{(g)} \rightleftharpoons CO_{(g)} + H_{2(g)}$

Consider the following reactions. In which cases is product formation favoured by decreased temperature?
$(a) \ N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}; \ \Delta H^o = 181 \ kJ$
$(b) \ 2CO_{2(g)} \rightleftharpoons 2CO_{(g)} + O_{2(g)}; \ \Delta H^o = 566 \ kJ$
$(c) \ H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}; \ \Delta H^o = -9.4 \ kJ$
$(d) \ H_{2(g)} + F_{2(g)} \rightleftharpoons 2HF_{(g)}; \ \Delta H^o = -541 \ kJ$

When in any system at equilibrium state,pressure,temperature,and concentration are changed,then the equilibrium shifts in such a direction as to neutralize the effect of the change. This is known as:

For a given equilibrium reaction,addition of inert argon gas at constant volume can shift the equilibrium in $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$