The equilibrium constant for a reaction is 10. What will be the value of `DeltaG^@ R= 8.314 Jk^-1 mol^(-1)` at T= 300K

The equilibrium constant (K_C) of a reversible reaction is 20.If the value of the forward rate constant is 320. the value of backward rate constant is

Calculate the standard entropy change for a reaction X rarr Y if the value of DeltaH^@ = +28.40 kJ and equilibrium constant is 1.8 xx 10-7 at 298 K.

The equilibrium constant (K_c) for the reaction N_2(g) + O_2 (g) rarr 2NO (g) at temperature T is 4xx10^(-4) .The value of K_c for the reaction, NO(g) rarr1//2 N_2 (g) +1//2O_2 (g) at the same temperature is:

The rate law for the reaction A+B rarr C is found to be rate = k [A]^2 [B] . The rate constant of the reaction at 25^@C is 6.25 M^(-2)S^(-1) . What is the rate of reaction, When [A] = 0.1 mol.dm^(-3) and [B] = 0.2 mol.dm^(-3) ?

What will be the value of pH of 0.01 mol dm^-3 CH_3COOH (K_a = 1.74 xx 10^-5) ?

The rate constant of a reaction is 2.1 xx 10^(-2) litre mol^(-1)s^(-1) . The order of reaction is

The energy of activation for a first order reaction is 104 kJ//mol . The rate constant at 25^@C is 3.7xx10^(-5)s^(-1) . What is the rate constant at 30^@C ? (R= 8.314 j//K mol) ]

Calculate the activation energy of a reaction for which rate constant becomes four times when temperature changes from 30^@C to 50^@C . Given : R=8.314 Jk^(-1) mol^(-1) .

At 700 K , equilibrium constant for the reaction, H_2(g) + I_2(g) hArr 2HI(g) is 54.8 if 0.5 mol L^(-1) of HI(g) is present at equilibrium at 700K,what are the concentration of H_2(g) and I_2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700K?

At a given temperature, the equilibrium constant for the reactions NO(g) +1/2O_2 (g) hArr NO_2(g) and 2NO_2 (g) hArr 2 NO (g) + O_2 (g) are K_1 and K_2 respectively.If K_1 is 4 xx 10^(-3) , then K_2 will be