Consider the partial decomposition of A as
`2A(g)hArr2B(g)+C(g)` At equilibrium 700 ml gaseous mixture contains 100 ml of gas C at 10 atm and 300 K. What is the value of `K_(P)` for the reaction?

Consider the pertial decomposition of A as 2A(g)hArr2B(g)+C(g) At equilibrium 700 mL gaseous mixture contains 100 mL of gas C at 10 atm and 300K what is the value of K_(p) for the reaction ?

Consider the pertial decomposition of A as 2A(g)hArr2B(g)+C(g) At equilibrium 700 mL gaseous mixture contains 100 mL of gas C at 10 atm and 300K what is the value of K_(p) for the reaction ?

Consider the pertial decomposition of A as 2A(g)hArr2B(g)+C(g) At equilibrium 700 mL gaseous mixture contains 100 mL of gas C at 10 atm and 300K what is the value of K_(p) for the reaction ?

Consider the partial decomposition of A as 2A_((g)) hArr 2B_((g)) + C_((g)) At equilibrium 700 m/ gaseous mixture contains 100 ml of gas C at 10 atm and 300K. What is the value of Kp for the reaction ?

For the reaction C(s) + CO_(2) (g) hArr 2CO(g). the partial pressures of CO_(2) and CO are 2.0 and 4.0 atm respectively at equilibrium. What is the value of K_(p) for this reaction?

At 207^@C , for the reaction : N_2(g) + 3H_2(g) hArr 2NH_3(g) it is found that at equilibrium, the mixture contains 52% of ammonia. If the pressure of the mixture is 10 atm, calculate K_p and K_c for the reaction.

For NH_(4)HS(s) hArr NH_(3)(g)+H_(2)S(g) , the observed, pressure for reaction mixture in equilibrium is 1.12 atm at 106^(@)C . What is the value of K_(p) for the reaction?

For NH_(4)HS(s) hArr NH_(3)(g)+H_(2)S(g) , the observed, pressure for reaction mixture in equilibrium is 1.12 atm at 106^(@)C . What is the value of K_(p) for the reaction?