At `1127K` and `1` atm pressure, a gaseous mixture of `CO` and `CO_(2)` in equilibrium with soild carbon has `90.55% CO` by mass
`C(s)+CO_(2)(g)hArr2CO(g)`
Calculate `K_(c)` for this reaction at the above temperature.

At 100 K the partial pressure of CO_(2) (g ) and CO (g) for the reaction CO_(2)(g) + C(s) hArr 2CO (g ) in a closed vessel at equilibrium are 0.15 and 0.60 bar respectively . The K_(c ) for this reaction at the same temperature is approximately

For the reaction CO_((g)) + Cl_(2(g)) hArr COCl_(2(g)). The K_(p)//K_(c) is equal to

For the equilibrium , 2NOCl(g)hArr2NO(g)+Cl_(2)(g) the value of the equilibrium constant, K_(c) is 3.75xx10^(-6) at 1069K . Calculate the K_(p) for the reaction at this temperature ?

A mixture of Na_(2)CO_(3) and K_(2)CO_(3) is used as fusion mixture because

C_((s))+O_(2(g))rarr CO_(2(g))+Q is ………………….

A mixture of one mole of CO_(2) and one mole of H_(2) attains equilibrium at a temperature of 250^(@)C and a total pressure of 0.1 atm for the change CO_(2(g)) +H_(2(g)) harr CO_((g))+H_(2)O_((g)) . Calculate K_(P) if the analysis of final reaction mixture shows 0.16 volume fraction of CO

For the reaction CO_((g))+CI_(2(g)) harr COCI_(2(g)) . The K_p // K_c is equal to

The reaction , CO(g)+3H_(2)(g)hArrCH_(4)(g)+H_(2)(g) is at equilibrium at 1300K in a 1L flask. It also contain 0.30 mol of CO , 0.10 mol of H_(2) and 0.02 mol of H_(2)O and an unknown amount of CH_(4) in the flask. Determine the concentration of CH_(4) in the mixture. The equilibrium constant. K_(c) for the reaction at the given temperature is 3.90 .