Write the expression for the equilibrium constant, 'K_c' for each of the following reactions:
i) '2 NOCl_(g)^ hArr 2 NO_(g)+Cl_2(g)'
ii) '2 Cu(NO_3)_(s) hArr 2 CuO_(s)^2+4 NO_2(g)+O_2(g)'
iii) 'CH_3 COOC_2 H_5(aq)+H_2 O_(l) hArr CH_3 COOH_(aq)+C_2 H_5 OH_(aq)'
iv) 'F e_( (aq) ^(3+)+3 OH_ (aq)^- hArr F e(O H)_3(s)'
v) 'I_2(s)+5 F_2 hArr 2 IF_5'

Write expressions for the equilibrium constance for the following reactions. CuO(s)+H_2(g)iff Cu(s)+H_2O(g)

Write the expression for equilibrium constant K_c for the following equilibrium. 2NOCl (g) harr 2NO (g) + Cl_2 (g)

Write the expression for equilibrium constant K_c for the following equilibrium. CuSO_4.5H_2O_(s) harr CuSO_4.3H_2O_(s) + 2H_2O_(g)

Write the expression for equilibrium constant K_Theta for the following equilibrium. CuSO_4 .5H_2O_((g))harr CuSO_4 .3H_2O_(s)+2H_2O_(g)

Write an expression for equilibrium constant, Kc f or the reaction, 4NH_3(g)+5O_2(g)harr 4NO(g)+6H_2O(g)

Write the expression for equilibrium constant K_p for the following equilibrium CuSO_4. 5H_2O_((s))iff CuSO_4 . 3H_2O_((s))+2H_2O_((g))

Write half equations for each of the following redox reactions: i) 'Zn(s)+PbCl_2(aq) rarr Pb(s)+ZnCI_2(aq)' ii) '2 Fe^(3+)(aq)+2 I-(aq) rarr I_2(aq)+2 Fe^(2+)(aq)' iii) '2 Na(s)+Cl_2(g) rarr 2 NaCl(s)'

At 1000K, equilibrium constant K_c for the reaction 2SO_3(g) harr 2SO_2(g)+O_2(g) is 0.027. What is the value of K_p at this temperature?

Which of the following reactions will get affected by increasing of pressure? Also mention whether change will cause the reaction to go into forward or backward direction? i) 'COCl_2(g) hArr CO_(g)+Cl_2(g)' ii) 'C H_4(g)+2 S_2(g) hArr CS_2(g)+2 H_2 S_(g)' iii) 'CO_2(g)+C_(s) hArr 2 CO_(g)' iv) '2 H_2(g)+CO_ th ) hArr CH_3 OH_(g)' 'v) CaCO_3(s) hArr CaO_(s)+CO_2(g)' vi) '4 NH_3( g)+5 O_2(g ) hArr 4 NO_(g)+6 H_2 O_(g'

Write the half reactions for the following redox reaction. Zn(s) + 2H^+ (aq) rarr Zn^(2+) (aq) + H_2(g)