The equilibrium constant for the following reaction is 10.5 at 500k. A system of equilibrium has CO=0.250M and `H_(2)` = 0.120M. What is the concentration of `CH_(3)OH` reaction `CO_(g)` + 2`H_(2g)` `CH_(3)OH`

The equilibrium constant for the following reaction is 10.5 at 500 K .A syatem at equilibrium has [CO]=0.250M and [H_(2)]=0.120 M "what is the "[CH_(3)OH] ? CO(g)+2H_(2)(g)hArrCH_(3)OH(g)

Which catalyst is used in the preparation of CH_(3)OH by the reaction of CO(g) & H_(2)(g) ?

Write the equilibrium constant expression for the following reactions : CH_4 (g) + 2O_2 (g)hArr CO_2(g)+ 2H_2O (g)

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

If helium gas is added at constant pressure to the following reaction at equilibrium CO(g) + 3H_2(g) hArr CH_4(g) + H_2O(g) , then

At 500 K, equlibrium constant, K_(c) for the following reaction is 5. 1//2 H_(2)(g)+ 1//2(g)hArr HI (g) What would be the equilibrium constant K_(c) for the reaction 2HI(g)hArrH_(2)(g)+l_(2)(g)

Calculate the equilibrium constant (K) for the formation of NH^ in the following reaction: N_2(g) + 3H_2(g) At equilibrium, the concentration of NH_3 , H_2 and N_2 are 1.2 xx 10^(-2) ,3.0 xx 10^(-2) and 1.5 xx 10^(-2) M respectively.

If the equilibrium constant of the reaction 2HIhArr H_(2)+I_(2) is 0.25, then the equilibrium constant for the reaction, H_(2)(g)+I_(2)(g)hArr 2HI(g) would be

The equilibrium constant for the reaction H_(2)O(g)+CO(g)hArrH_(2)(g)+CO_(2)(g) is 0.44 at 1660 K. The equilibrium constant for the reaction 2H_(2)(g)+2CO_(2)(g)hArr 2CO(g)+2H_(2)O(g) at 1660 K is equal to

Form the given data of equilibrium constants of the following reactions: CuO(s)+H_(2)(g)hArrCu(s)+H_(2)O(g),K=67 CuO(s)+CO(g)hArrCu(s)+CO_(2)(g),K=490 Calculate the equilibrium constant of the reaction, CO_(2)(g)+H_(2)(g)hArr+CO(g)+H_(2)O(g)