Expression OF Kp/Kc || Case 1st :- Homogeneous Gaseous Reaction (a) Δng=0 (b) Δng>0 (c) Δng<0 || Solved Numerical Class illustration"

log K_p/K_c +log RT=0 is a relationship for the reaction :

The synthesis of HBr from hydrogen and liquid bromine has an equilibrium constant Kp = 4.5×x10^(15) at 25°C. Given that the vapor pressure of liquid bromine is 0.28 atm, find Kp for the homogeneous gas-phase reaction at the same temperature.

For a reaction, aA+bBhArrcC+dD , the reaction quotient Q=([C]_(0)^(c)[D]_(0)^(d))/([A]_(0)^(a)[B]_(0)^(b)) , where [A]_(0) , [B]_(0) , [C]_(0) , [D]_(0) are initial concentrations. Also K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)) where [A] , [B] , [C] , [D] are equilibrium concentrations. The reaction proceeds in forward direction if Q lt K_(c) and in backward direction if Q gt K_(c) . The variation of K_(c) with temperature is given by: 2303log(K_(C_(2)))/(K_(C_(1)))=(DeltaH)/(R)[(T_(2)-T_(1))/(T_(1)T_(2))] . For gaseous phase reactions K_(p)=K_(c)(RT)^(Deltan) where Deltan= moles of gaseous products - moles of gaseous reactants. Also -DeltaG^(@)=2.303RT log_(10)K_(c) . Which relation is correct?

In the case of gaseous homogeneous reaction, the active mass of the reaction is obtained by the expression.

Write expressions for K_p and K_c for the decomposition reaction of calcium carbonate.

For which reaction does K_p=K_c ?