Calculate partial pressure of B at equilibrium in the following equilibrium
`A(s) iff B(g) +2C(g), " " K_(P)=32 atm^(3)`.

At 46^@C, K_p for the reaction N_2O_4(g) iff 2NO_2(g) is 0.66. Calculate the partial pressure of N_2O_4 and NO_2 at equilibrium and at a total pressure of 0.5 atm.

A sample of HI (g) is placed in a flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI (g) is 0.04 atm. What is K_(p) for the given equilibrium ? 2HI(g) hArr H_(2)(g) + I_(2)(g)

The equilibrium partial pressures of CO(g), CO_(2)(g) in the equilibrium reaction CO_(2)(g)+C(s) iff 2CO(g) at 1000 K are 0.66 and 0.15 bar respectively. The equilibrium constant K_(c) are apporximately is

A vessel at 1000K contains CO_(2)(g) at 2 atm pressure. When graphite is added the following equilibrium is established. CO_(2)(g)+C(s) hArr 2CO(g) the toal pressure at equilibrium is 3 atm. The value of K_(p) is

A vessel at 1000K contains CO_(2)(g) at 2 atm pressure. When graphite is added the following equilibrium is established. CO_(2)(g)+C(s) hArr 2CO(g) the toal pressure at equilibrium is 3 atm. The value of K_(p) is

A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium, the partial pressure of HI(g) is 0.04 atm. What is K_p for the equilibrium 2HI(g) iff H_2(g)+I_2(g)

A sample of HI(g) is placed in flask at a pressure of 0.2 atm . At equilibrium. The partial pressure of HI(g) is 0.04 atm . What is K_(p) for the given equilibrium? 2HI(g) hArr H_(2)(g)+I_(2)(g)