`CaCO_3(s) For the given reaction at equilibrium, prove that `pco_2` always has a fixed value at a particular temperature and it is independent of the amount of `CaCO_3(s)`

At a given temperature, the equilibrium constant K_c for the reaction, A+BtoC is 10. At the same temperature the reaction is allowed to occur in a closed vessel of volume 1L. At a particular moment of time during the reaction, if the amount of A, B and C in the reaction system are 0.1,0.4 and 0.3 mol respectively then-

The reaction C(s)+CO_2(g)hArr2CO_2(g) is in a state of equilibrium in a closed vessel at a constant temperature. The equilibrium of the reaction will shift towards left and get re-established if at constant temperature and volume some amount of-

The given reaction is carried out in a closed vessel: CaCO_(3)(s)hArr CaO(s)+CO_(2)(g), DeltaH^(0) gt0 . What would be the effect of the following changes on the equilibrium of the reaction if (1) solid CaCO_(3) is added to the reaction system, (2) some amount of CaO is removed from the reaction system, (3) CO_(2)(g) is introduced into the reaction system at constant volume and temperature., (4) temperature is increased, and (5) volume of the reaction vessel is reduced at constant temperature.

The given graph indicates the change in concentrations of A and B of a reversible reaction, A hArr nB at constant temperature. If the value of equilibrium constant of the reaction is 1.2 at that temperature, then find the value of n.

What amount of CaCO_(3) will be just sufficient to produce 1 L of CO_(2) at 27^(@)C and 760 mmHg pressure? Determine the quantity of pure carbon requried to yield the same amount of CO_(2) .

If 20 g of CaCO_3 is treated with 100 mL of 20% HCl solution, the amount of CO_2 produced is