For the reaction, C(s)+CO2(g)⇌2CO(g), the partial pressure of CO2 and CO are 2.0 and 4.0 atm, respectively. At equilibrium what is the value of Kp for this reaction?

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO is 2.0 and 4.0 atm, respectively, at equilibrium. The K_(p) of the reaction is

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO is 4.0atm amd 8.0 atm, respectively, at equilibrium. The K_(p) of the reaction is

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO is 5.0atm amd 10 atm, respectively, at equilibrium. The K_(p) of the reaction is

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO both is 4.0 atm, respectively, at equilibrium. The K_(p) of the reaction is

For the reaction C(s)+CO_(2)(g) hArr 2CO(g) , the partial pressure of CO_(2) and CO both is 5.0 atm, respectively, at equilibrium. The K_(p) of the reaction is

For the reaction CaCO_3(s) hArr CaO(s) +CO_2(g) , the pressure of CO_2 depends on

For the reaction, N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) the partial pressure of N_(2) and H_(2) are 0.80 and 0.40 atmosphere, respectively, at equilibrium. The total pressure of the system is 2.80 atm. What is K_(p) for the above reaction?

For the reaction A_(2)(g) + 2B_(2)hArr2C_(2)(g) the partial pressure of A_(2) and B_(2) at equilibrium are 0.80 atm and 0.40 atm respectively. The pressure of the system is 2.80 atm. The equilibrium constant K_(p) will be

For the reaction , CO(g)+Cl(g)hArrCOCl_2(g) then K_p//K_c is equal to :

The partial pressures of NO , Br_2 , and NOBr in a flask at 25^@C are 0.01, 0.1 , and 0.04atm , respectively. If the equilibrium constant at 25^@C for the reaction 2NO(g)+Br_2(g)hArr 2NOBr(g) is equal to 160atm^(-1) , then we can say that