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)`

Write the expression for the equilibrium constant, K_C for each of the following reactions: 2NOCI(g) hArr 2NO (g) + CI_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 the expression for the equilibrium constant, K_C for each of the following reactions: Fe^(3+) (aq) + 3OH(aq) hArr Fe(OH)_3(s)

Write the expression for the equilibrium constant, K_C for each of the following reactions: CH_3COOC_2H_5(aq)+H_2O(l) hArr CH_3COOH(aq) + C_2H_5OH(aq)

Express the rate of a reaction in terms of concentration of each constituent in the following reaction. H_2(g) + I_2(g)rarr 2HI_((g))

Identify the molecularity and write the rate law for each of the following elementary reactions : H_(2(g)) + I_(2(g))rarr2HI_(g)

A mixture of 1.57 mol of n_2 ,1.92 mol of H_2 and 8.13 mol of NH_3 is introduced into a 20 L reaction vessel at 500 kAt this temperature,the equilibrium constant. K_C for the reaction N_2(g) + 3H_2(g) hArr 2NH_3(g) is 1.7 xx 10 ^2 .Is the reaction mixture at equilibrium?If not,what is the direction of the net reaction?

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

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

Justify the following reactions are redox reactions : 2K(s) + F_2 (g) rarr 2K^+F^- (s)