For the following reaction, the value of `K` change with
`N_(2)(g)+O_(2)(g) lt lt 2NO(g), DeltaH=+180 kJ mol^(-1)`

Assume DeltaH^(@) and DeltaS^(@) to be independent of temperature, at what temperature with the reaction given below becomes spontaneous? N_(2)(g) + O_(2)(g) to 2NO(g) DeltaH^(@) = 180.8 kJ mol^(-1)

Which of the following is not true for the equilibrium reaction N_2(g)+O_2(g)hArr 2NO(g) , DeltaH=180kJmol^(-1)

What would the effect on the yield of products be if temperature of the following reaction systems is changed at equilibrium ? (1) N_(2)(g)+O_(2)(g)hArr 2NO(g),DeltaH gt0 (2) 2SO_(2)(g)+O_(2)(g) hArr 2SO_(3)(g),DeltaH lt 0

Calculate the value of equilibrium constant, K for the following reaction at 400 K. 2NOCl(g) hArr 2NO (g) + Cl_2(g) DeltaH^@ = 80.0 kJ mol^(-1), DeltaS^@ = 120 KJ^(-1) mol^(-1) at 400 K, R = 8.31 JK^(-1) mol^(-1) .

Calcutate Delta H in kJ for the following reaction C(g)+O_(2)(g) Given that , H_(2)O(g)+C_(g)toCO(g)+H_(2)(g),""""" DeltaH=+131kJ CO(g)+(1)/(2)O_(2)(g)toCO_(2)(g) """"'DeltaH=-282kJ H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(g) """""DeltaH=-242kJ

Comment on the thermodynamic stability of NO(g), (given) N_2(g) + O_2(g) rarr 2NO(g) Delta H = 180KJ mol^(-1) 2NO(g) + O_2(g) rarr 2NO_2(g) Delta H = -148KJ mol^(-1)