`Kp//Kc` for `CO+frac(1)(2)O_2=CO_2`

Find out K_p//K_c for: CO(g)+frac 1/2 O_2 (g) overset (rarr)(larr) CO_2 (g) .

If mol*L^(-1) and 'atm' be the units of concentration and pressure respectively, then what will be the value of K_p//K_c for the reaction, N_2O_4(g)

Find out K_(p)//K_(c) for the reactio CO(g)+(1)/(2)O_(2)(g)hArr CO_(2)(g) .

At 25^@C the value of K_c , for the reaction 1/2N_2+O_2iffNO_2 is 2xx10(-4) , what will be the value of K_c for 2NO_2iffN_2+2O_2

Establish the relation between K_p and K_c for the reaction 2SO_2(g)+O_2(g)iff2SO_3(g)

Calculate the molar mass: (1) H_(2)O (2) CO_(2)

The equilibrium constant (K_c) for the reaction N_2(g)+O_2(g)to2NO(g) at temperature T is 4xx10^(-4) The value of K_c for NO(g)to1/2N_s(g)+1/2O_2(g) at the same temperature is

Simplify - (xii) 1frac(1)(2) [ 3frac(1)(2) + 2frac(1)(3) { 1frac(1)(4) + (2+ 3frac(2)(3) )}]

Calculate the value of K_c for the given reactions: N_2O_4(g)hArr 2NO_2(g),K_p=11 ( at 100^(@)C )

Calculate the standard enthalpy of reaction at 25^@C temperature for the following reaction : C_6H_6(I) + frac 15/2 O_2 (g) rarr 6CO_2(g)+3H_2O(I) . Given: The standard enthalpy of formation of C_6H_6(I) , .CO_2(g) and H_2O(I) are 49.0kJ mol^-1 , -393.5 kJ mol^-1 and -285.8 kJ mol^-1 respectively.