For a water gas reaction `C(s) + H_2O(g) harr CO(g) + H_2(g) at 1000^@C`, the standard Gibb's energy change is `-8.1 KJ mol^(-1)`. Calculate the value of equilibrium constant.

Dihydrogen gas used in Haber's process is produced by reacting methane form natural gas with high temperature steam..The first stange reaction involves the formation of CO and H_2 .In second stage , CO formed in first stage,CO formed in first stage is reacted with more steam ion water gas shift reaction, CO(g)+ h_2o(g) hArr CO_2(g) +H_2(g) If a reaction vessel at 400^@C is charged with a n equimolar mixture of CO and steam such that P_(co) =P_(H_2O) = 4.0 bar what will be the partial pressure of H_2 at equilibrium? k_p =0.1

The enthalpy changes for the reaction C_2H_4(g) + H_2(g) rarr C_2H_6(g) is -620J When 100ml of ethylene and 100ml of H_2reacts at 1 bar pressure. Calculate the pressure volume type of work and DeltaU for the reaction

For the reaction C_(3)H_(8)(g)+5O_(2) (g)rarr3CO_(2)(g)+4H_(2)O(l) at constant temperature, DeltaH-DeltaU is

For the reaction, C_2H_4(g) + H_2(g)rarr C_2H_6(g), K_p= 3.356 xx 10^(17) Calculate Delta G° for the reaction at 25^@C .

One mole of H_2O and one mole of CO are taken in 10L vessel and heated to 725 K.At equilibrium 40% of water (by mass) reacts with CO according to the equatin H_2O(g0 + CO(g) hArr H_2(g) +CO_2(g) Calculate the equilibrium constant for the reaction.

Ammonia and oxygen react at high temperature as : 4 NH_(3(g)) + 5O_2(g)rarr 4NO(g) + 6H_2O_(g) In an experiment, rate of formation of NO(g) is 3.6 xx 10^(-3) mol L^(-1). s^(-1) Calculate :-Rate of formation of water.