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?

At '473 K', equilibrium constant Kc for decomposition of phosphorus pentachloride 'PCl_5' is '8.3 xx 10^(-3) .' If decomposition is depicted as, 'PCl_5(g) hArr PCl_3(g)+Cl_2(g) , Delta, H^circ=124.0 kJmol^(-1)' a. write an expression for 'K_c' for the reaction b. what is the value of 'K_c' for the reverse reaction at the same temperature? c. what would be the effect on 'K' c if (i) more 'PCl_5' is added (ii) pressure is increased. (iii) the temperature is increased?

Assume that the reaction given below is at equilibrium. PCl_(5(g)) harr PCl_(3(g)) + Cl_(2(g)) , DeltaH = 124.0 Kjmol^-1 . Explain, how the following changes influence this equilibrium. increase in temperature.

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

For the reaction PCl_5 harr PCl_3 + Cl_2 Write the expression of Kc'

Assume that the reaction given below is at equilibrium. PCl_(5(g)) harr PCl_(3(g)) + Cl_(2(g)) , DeltaH = 124.0 Kjmol^-1 . Explain, how the following changes influence this equilibrium. increase in pressure

Assume that the reaction given below is at equilibrium. PCl_(5(g)) harr PCl_(3(g)) + Cl_(2(g)) , DeltaH = 124.0 Kjmol^-1 . Explain, how the following changes influence this equilibrium. Addition of neon gas at constant volume.

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?

Consider a reaction PCl_5(g) rarr PCl_3(g)+Cl_2(g) b) Explain why does PCl_5 decomposes easily?