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)`

The equilibrium constant for the following reactoin is 10 at 500 K.A system at equilibrium has [CO] = 0.25M and [H_(2)] 1M.What is the [CH_(3)OH] ? CO_((g))+2H_(2(g))hArrCH_(3)OH_((g)) CO_((g))+2H_(2(g))hArrCH_(3)OH_(g)

For the reaction : CO(g)+2H_(2)(g)hArr CH_(3)OH(g)

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

The equilibrium constant for the following reactions at 1400 K are given. 2H_(2)O(g)hArr2H_(2)(g) + O_(2)(g) , K_(1)=2.1×x10^(-13) 2CO_(2)(g) hArr2CO(g)+O_(2)(g),K_(2) = 1.4 x× 10^(-12) Then, the equilibrium constant K for the reaction H_(2)(g) + CO_(2)(g)hArrCO(g) + H_(2)O(g) is

The equilibrium constant of the following reactions at 400 K are given: 2H_(2)O(g) hArr 2H_(2)(g)+O_(2)(g), K_(1)=3.0xx10^(-13) 2CO_(2)(g) hArr 2CO(g)+O_(2)(g), K_(2)=2xx10^(-12) Then, the equilibrium constant K for the reaction H_(2)(g)+CO_(2)(g) hArr CO(g)+H_(2)O(g) is

The equilibrium constant of the equilibrium equation H_2O(g)+CO(g)hArrH_2(g)+CO_2(g) is 0.44 at 1259K . The value of equilibrium constant for the equilibrium equation H_2(g)+2CO_2(g)hArrH_2O(g)+CO(g) will be