For the reaction `H_2(g)+I_2(g) hArr 2 HI (g)`
`K c=54.8` at `700 K .` Calculate the value of `K_p`

For the reaction, H_2(g) + I_2(g) harr 2HI(g) , value of K_c is 46.4 at 298K. What is the value of Kp?

The equilibrium constant of the reaction H_2(g) + I_2(g) harr 2HI(g) is 57 at 700 K. Now, give the equilibrium constants for the following reaction at the same temperature: 4HI(g) harr 2H_2(g) +2I_2(g)

Equilibrium constant 'K_c' for the reaction 'N_2(g)+3 H_2(g) hArr 2 N H_3(g)' at '500 K' is '0.061' At a particular time, the analysis shows that composition of the reaction mixture is '3.0 molL^(-1) N_2, 2.0' mol 'L^(-1) . H^2' and '0.5 mol L^(-1) NH_3 .' Is the reaction at equilibrium? If not in which direction does the reaction tend to proceed to reach equilibrium?

The activation energy for the reaction, 2HI(g)toH_2(g)+I_2(g) is 209.5kj mol^(-1) at 581 K.Calculate the fraction of molecules of reactant having energy equal to or greater than activation energy.

For a gaseous reaction: 2 X(g) hArr 2 Y(g)+Z(g) , K_p=1.8 at 700^(circ)C . The value of K_(c) for the reaction : 2 Y(g)+Z(g) hArr 2 X(g) at 44.4 33.1 1.3×10^(−3) 0.031