What is`K _C` for the following equilibrium when the equilibrium concentratin of each substane is `[SO_2]=0.60 M,[O_2]=0.82 M` and `[SO_3] =1.90 M? 2SO_2(g) + o_2(g) hArr 2SO_3(g)`

What is the equilibrium concentration of each of the substances in the equilibrium when the intial concentration of ICI was 0.78 M? 2ICI(g) hArr I_2(g) + CI_2 (g),K_C =0.14

K_p =0.04 at 899 K for the equilibrium shoen below.What is the equilibrium concentration of C_2H_6 when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium? C_2H_6(g) hArr C_2H_4(g) +H_2(g)

Write the expression for the equilibrium constant, K_C for each of the following reactions: 2Cu(NO_3)_2 hArr 2CuO(s) + 4 NO_2(g)

Write expressions of k_c for following chemical reactions. 2SO_2(g) + O_2(g) harr 2SO_3(g) .

Write the expression for the equilibrium constant, K_C for each of the following reactions: 2NOCI(g) hArr 2NO (g) + CI_2(g)

The elementary reaction O_3(g) + O(g) rarr 2 O_2(g) is

Write the expression for the equilibrium constant, K_C for each of the following reactions: I_2(s) +5F_2(g) hArr 2IF_5(l)

Answer the following questions: Classify the following oxide into three types and name the types. CaO, MgO, CO_2 , SO_3 , Na_2 O , ZnO, Al_2 O_3 , Fe_2 O_3

At a given temperature, the equilibrium constant for the reactions NO(g) +1/2O_2 (g) hArr NO_2(g) and 2NO_2 (g) hArr 2 NO (g) + O_2 (g) are K_1 and K_2 respectively.If K_1 is 4 xx 10^(-3) , then K_2 will be

For the system A (g) + 2 B (g) hArr C(g) the equilibrium concenrations are A =0.06 mol L^(-1) B = 0,12 mol L^(-1) C = 0.216 mol L^(-1) The K_(eq) for the reaction is