Write the expression for the equilibrium constant- Kc for each of the following reactions-i 2 NOCl g - 2 NO g - Cl 2 g ii 2 Cu NO 32 aq - 2 CuO S -4 NO 2 g - O 2 g iii CH 3 COOC 2 H 5 aq - H 2 O l - CH 3 COOH aq - C 2 H 5 OH aq iv F e 3- aq -3 OH - aq - Fe OH 3 s v I 2 s -5 F 2- 2 IF 5

Name: NCERT - Grade 11 - Chemistry - Equilibrium - Q32_02
Uploaded: 2022-07-04T10:36:42+05:30
Description: (i) K_c=[NO_g]^2[Cl_2(g)]/[NOCl_g]^2 (ii) K_c=[CuO_(s)]^2[NO_2(g)]^4[O_2(g)]/[Cu(NO_3)_2(aq)] =[NO_2(g)]^4[O_2(g)]/[Cu(NO_3)_2(aq)] (iii) K_C[CH_3COOH_(aq)][C_2 ...

(i) K_c=[NO_g]^2[Cl_2(g)]/[NOCl_g]^2 (ii) K_c=[CuO_(s)]^2[NO_2(g)]^4[O_2(g)]/[Cu(NO_3)_2(aq)] =[NO_2(g)]^4[O_2(g)]/[Cu(NO_3)_2(aq)] (iii) K_C[CH_3COOH_(aq)][C_2 ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Derivation of Kp and Kc

Write the exp...

Question

Write the expression for the equilibrium constant, $K_{C}$ for each of the following reactions:

(i) $2 N O C l (g) \leftrightarrow 2 N O (g) + C l_{2} (g)$

(ii) $2 C u (N O_{3})_{2} (a q) \leftrightarrow 2 C u O (S) + 4 N O_{2} (g) + O_{2} (g)$

(iii) $C H_{3} C O O C_{2} H_{5} (a q) + H_{2} O (l) \leftrightarrow C H_{3} C O O H (a q) + C_{2} H_{5} O H (a q)$

(iv) $F e^{3 +} (a q) + 3 O H^{-} (a q) \leftrightarrow F e (O H)_{3} (s)$

(v) $I_{2} (s) + 5 F_{2} \leftrightarrow 2 I F_{5}$

Open in App

Solution

The expression for the equilibrium constant, $K_{C}$ for each of the following reactions are:
(i) $K_{c} = \frac{[N O]^{2} [C l_{2}]}{[N O C l]^{2}}$

(ii) $K_{c} = \frac{[C u O]^{2} [N O_{2}]^{4} [O_{2}]}{[C u (N O_{3})_{2}]}$
= $\frac{[N O_{2}]^{4} [O_{2}]}{[C u (N O_{3})_{2}]}$

(iii) $K_{C} = \frac{[C H_{3} C O O H] [C_{2} H_{5} O H]}{[C H_{3} C O O C_{2} H_{5}] [H_{2} O]} = \frac{[C H_{3} C O O H] [C_{2} H_{5} O H]}{[C H_{3} C O O C_{2} H_{5}]}$

(iv) $K_{C} = \frac{[F e {(O H)}_{3}]}{[F e^{3 +}] {[O H^{-}]}^{3}} = \frac{1}{[F e^{3 +}] {[O H^{-} (a q)]}^{3}}$

(v) $K_{C} = \frac{{[I F_{5}]}_{5}^{2}}{[I_{2} (s)] {[F_{2}]}_{2}^{5}} = \frac{{[I F_{5}]}_{5}^{2}}{{[F_{2}]}_{2}^{5}}$

Suggest Corrections

Similar questions

Q. Write the expression for the equlibrium constant,

K_{c}

for each of the following reactions.
(i)

2 N O C l (g) \to 2 N O (g) + C l_{2} (g)

(ii)

2 C u (N O_{3})_{2} (s) \to 2 C u O (s) + 4 N O_{2} (g) + O_{2} (g)

(iii)

C H_{3} C O O C_{2} H_{5} (a q) + H_{2} O (l) \to C H_{3} C O O H (a q) + C_{2} H_{5} O H (a q)

(iv)

F e^{3 +} (a q) + 3 O H^{-} (a q) \to F e (O H)_{3} (s)

(v)

I_{2 (s)} + 5 F_{2} (g) \to 2 I F_{5} (g)

Predict which of the following reaction will have appreciable concentration of reactants and products:
a) $C l_{2} (g) \leftrightarrow 2 C l (g); K_{c} = 5 \times 10^{- 39}$
b) $C l_{2} (g) + 2 N O (g) \leftrightarrow 2 N O C l (g); K_{c} = 3.7 \times 10^{8}$
c) $C l_{2} (g) + 2 N O_{2} (g) \leftrightarrow 2 N O_{2} C l (g); K_{c} = 1.8$

Which of the following reactions will get affected by increasing the pressure?
Also, mention whether change will cause the reaction to go into forward or backward direction.
(i) $C O C l_{2} (g) \leftrightarrow C O (g) + C l_{2} (g)$
(ii) $C H_{4} (g) + 2 S_{2} (g) \leftrightarrow C S_{2} (g) + 2 H_{2} S (g)$
(iii) $C O_{2} (g) + C (s) \leftrightarrow 2 C O (g)$
(iv) $2 H_{2} (g) + C O (g) \leftrightarrow C H_{3} O H (g)$
(v) $C a C O_{3} (s) \leftrightarrow C a O (s) + C O_{2} (g)$
(vi) $4 N H_{3} (g) + 5 O_{2} (g) \leftrightarrow 4 N O (g) + 6 H_{2} O (g)$

Find out the value of K_c for each of the following equilibria from the value of $K_{p}$ :
(i) $2 N O C l (g) \leftrightarrow 2 N O (g) + C l_{2} (g) : K_{p} = 1.8 \times 10^{- 2} a t 500 K$