2 N O C l g ↔ 2 N O g + C l 2 ( g ) .Find the value of `K_c` for above equilibrium if the value of `K_p` is `1.8xx10^2` atm at 600 K. `[R = 0.082 L atm//K//mol]`

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

Find out the value of K_c for each of the following equilibria from the value of K_p 2NOCl(g)iff2NO(g)+Cl_2(g),K_p=1.8xx10^-2 at 500 K

Find out the value of K_c for each of the following equilibria from the value of K_p CaCO_3(s)iff CaO(s)+CO_2(g),K_p=167 at 1073 K

The volume of 2.8g of CO at 27°C and 0.821 atm pressure is (R = 0.0821 l atm Km^(-)ol^(-) )

5.1 g of solid NH_(4)SH is introduced into a evacuated 3L flask at 600 K. 30% of the NH_(4)SH dissociated into NH_(3) and H_(2)S gases by the time equilibrium is reached. The K_(p) of the reaction at 600 K is (R = 0.082 L atm mol^(-1)K^(-1), N=14, S=32 )