At 700 K, `CO_2` and `H_2` react to form CO and `H_2O`. For this process K is 0.11. A mixture of 0.45 mole of `CO_2` and 0.45 mole of `H_2` is heated to 700 K, then Find out the amount of each gas at equilibrium.

At 700 K, CO_2 and H_2 react to form CO and H_2O . For this process K is 0.11. [fa mixture of 0.45 mole of CO_2 and 0.45 mole of H_2 is heated to 700 K, then After equilibrium is reached another 0.34 mole of CO_2 and 0.34 mole of H_2 are added to the reaction mixture. Find the composition of the mixture at the new equilibrium state. (Assume volume to be 1 dm^3 )

Calculate the partial pressures of O_2 and H_2 in a mixture of 3 moles of O_2 and 1 mole of H_2 at S.T.P.

Calculate the partial pressures N_2 and H_2 in a mixture of two moles of N_2 and two moles of H_2 at STP.

A vessel at 1000K contains CO_2 with a pressure of 0.5 atm. Some of the CO_2 is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8atm. The value of K is

In a gas mixture of H_(2) and He , the partial pressure of H_(2) is half that of He. Find the mole fractions of H_(2) and He in the mixture.

One mole of H_2 , 2 moles of I_2 and 3 moles of HI are injected in a one litre of flask. What will be the concentration of H_2, I_2 and HI at equilibrium when K_c is 45.9 ?

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.

Draw Z vs P for H_2 and CO_2 at 0^@C