For the equilibrium `2NO_(2)(g)hArrN_(2)O_(4)(g) + 14.6` Kcal the increase in temperature would

For the equilibrium reaction 2NO_2(g) hArr N_2O_4(g) + 60.0 kJ the increase in temperature

For the equilibrium 2NO_2(g) ⇌ N_2O_4(g) +14.6 kcal An increase of temperature will:

For the reaction 2NO_(2(g))hArrN_(2)O_(4(g)),K_(p)//K_(c) is equal to

For the reaction 2NO_(2(g))hArrN_(2)O_(4(g)),K_(p)//K_(c) is equal to

For the equilibrium equation 2NH_3(g)hArrN_2(g)+3H_2(g) the units of K_p will be

The equilibrium constant for the reaction 2NO_(2)(g)iff2NO(g)+O_(2)(g)" is "2xx10^(-6)" at "185^(@)C . Then the equilibrium constant for the reaction, 4NO(g)+2O_(2)(g)rarr2NO_(2)(g) at the same temperature would be

For the reaction, CO_((g))+H_(2)O_((g))hArrCO_(2(g))+H_(2(g)) at a given temperature, the equilibrium amount of CO_(2(g)) can be increased by:

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) at temperature T is 4xx10^(-4) . The value of K_(c) for the reaction NO(g) hArr 1/2 N_(2)(g)+1/2 O_(2)(g) at the same temperature is