For the equilibrium `2SO_3(g) to 2So_2(g)+O_2(g), K_c` at 47^0C 3.25xx10_-9` mol per liter. What will be the value of `K_p` at this temperature(R=`8.314 JK_1mol_1`)

2SO_3(g) harr 2SO_2(g) + O_2(g) For the equilibrium K_c at 470^@C is 3.25xx10^-9 mol//lit . What will be the value of K_p at this temperature?

At 1000K, equilibrium constant K_c for the reaction 2SO_3(g) harr 2SO_2(g)+O_2(g) is 0.027. What is the value of K_p at this temperature?

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 equilibrium, PCl_(5(g)) rarr PCl_(3(g)) + Cl_(2(g)) , (K = 1.8x10^-7) . DeltaG^0 for the reaction at 298K?

Write the expression for equilibrium if the value of K_p for the following equilibrium. 2NOCl_(g) harr2NO_(g) + Cl_2(g). find the value of K_c for above equilibrium if the value of K_p is 1.8xx10^-2 atm at 600K. R=0.0821L atm K_1 mol_1

a) State Hess's Law of constant heat summation. b) The equilibrium constant for a reaction is 5. What will be tha value of DeltaG^0. Given that R = 8.314 JK^-1mol^-1 , T=300K. R = 8.314 JK^-1mol^-1 T = 300K

The K_c for the following reaction. PCl_(5(g)) harr PCl_(3(g)) + Cl_2(g) , H = 124.0 kJ mol^-1 is 8.3xx10^14 .What is the value of Kc for the reverse reaction at the same temperature?

The equilibrium constant for the equilibrium PCl_(5)(g) hArr PCl_(3)(g) + Cl_(2)(g) at a particular temperature is 2 xx 10^(-2)" mol dm"^(-3) . The number of moles of PCI_(5) that must be taken in a one-litre flask at the same temperature to obtain a concentration of 0.20 mol of chlorine at equilibrium is