`A_(2)(g)+B_(2)(g)hArr 2AB(g),` equilibrium constant of the given reaction at `100^(@)C` is 50. A 1 L flask containing 1 mol of `A_(2)` is connected to a 2L flask containing 2mol of `B_(2)`. Calculate theno. Of moles of AB at `100^(@)C` at equilibrium.

A_2(g)+B_2(g)

The unit of equilibrium constant of the reaction, A+3B hArr nC is L^(2)*mol^(-2) . What is the value of n

The reaction CO(g)+3H_(2)(g) hArr CH_(4)(g)+H_(2)O(g) is at equilibrium at 1300K in a 1L flask. It also contains 0.30 mol of CO, 0.10 mol of H_(2) and 0.02 mol of H_2O and an unknown amount of CH_(4) in the flask. Determine the concentration on CH_(4) in the mixture. the equilibrium constant, K_(c) for the reaction at the given temperature is 3.90.

A 2L flask contains 0.4 g O_(2) and 0.6 g H_(2) at 100^(@)C . Calculate the total pressure of the gas mixture in the flask.

At 100^(@)C a 2 litre flask contains 0.4 g of O_(2) and 0.6 g of H_(2) . What is the total pressure of this gas mixture in the flask?

The equilibrium constant for the reaction , 1/2H_2(g)+1/2I_2(g)toHI(g) is K_c then find equilibrium constant for 2HI(g)toH_2(g) + I_2(g)

AB(g)+1/2B_2(g) rarr AB_2(g) , equilibrium constant =K_1 2AB_2(g)rarr2AB(g)+B_2(g) , equilibrium constant =K_2 . Find the relation between K_1 and K_2

At 986^(@) C the value of equilibrium constant (K_c) for the reaction, CO(g)+H_2O(g)toCO_2(g)+H_2(g) is 0.63At this temperature, 1 mol of H_2O (g) is allowed to react with 3 mol of CO(g). This results in the above equilibrium in which the observed pressure is 2.0 atm. Find the number of moles of H_2 (g) produced at equilibrium and the partial pressure of each gas

At a certain temperature, the equilibrium constant K_c is 16 for the reaction, SO_2(g) + NO_2(g) iff SO_3(g) + NO(g) . If 1.0 mol each of all the four gases is taken in a one litre container the concentration of NO_2 at equilibrium would be