At 1127 K and 1 atm pressure , a gaseous mixtue of CO and `CO_2` in equilibrium with solid carbon has 90.55% CO by mass `C(s) + CO_2 hArr 2CO(g)`Calculate `K_c` for this reaction at the above temperature.

If the pressure and absolute temperature of 2 litres of CO_2 are doubled, the volume of CO_2 would becomes.

The pressure and temperature of 4 dm^3 of CO_2 gas are doubled,the volume of CO_2 gas would be

At a certain temperature and total pressure of 10^5 Pa,iodine vapour contains 40% by volume of 1 atoms I_2(g) hArr 2I(g) Calculate K_p for the equilibrium.

K_p for the reaction, MgCO_(3(s)) rarr MgO_((s)) + CO_(2(g)) is 9 xx 10^(-10) . Calculate DeltaG^@ for the reactionat 25^@C .

One mole of H_2O and one mole of CO are taken in 10L vessel and heated to 725 K.At equilibrium 40% of water (by mass) reacts with CO according to the equatin H_2O(g0 + CO(g) hArr H_2(g) +CO_2(g) Calculate the equilibrium constant for the reaction.

The reaction, CO(g) + 3H_2 (g) hArr CH_4(g) + H_2O(g) is at equilibrium at 1300K in a 1L.flask.If also contain 0.30 mol of CO. 0.10 mol of H_2 and 0.02 mol of H_2O and unkown amount of CH_4 in the flask.Determine the concentration of CH_4 in the mixture. The quilibrium constant. K_c for the reacton at the given temperature is 3.90.

Critical temperature of CO_2(g) is

Describe the effect of :removal of CO on the eauilibrium of the reaction, 2H_2(g) + CO(g) hArr CH_3OH(g)

In the equilibrium reaction involving then diansociation of CaCO_3(s) : CaCO_3(s) hArr CaO (s) + CO_2 (g) , the equilibrium constant is given by

Find out the value of K_c for each of the following equilibria from the value of K_p : CaCO_3 (s) hArr CaO(s) + CO_2(g) , K_p=167 at 1073 K