Find the value of Kc if Kp for the given reaction is 1-8- 10-2 at 500K 2NOCl- 2NO-Cl2-

2NOCl (g) ⇌ 2NO + Cl_2 Δ n_g = 3 2 = 1 Kp = Kc (RT)^Δ n = #160; Kc =Kp/RT #160; #160; #160;= 1.8× 10^ 2/0.0831× 500 = 4.33× 1 ...

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Characteristics of Equilibrium Constant

Find the valu...

Question

Find the value of Kc if Kp for the given reaction is $1.8 \times 10^{- 2}$ at $500$ K $2 N O C l ⇌ 2 N O + C l_{2}$ .

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K_{c}

(i) 2 N O C l (g) ⇌ 2 N O (g) + C l_{2} (g); K_{P} = 1.8 \times 10^{- 2} a t 500 K

(i i) C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g); K_{p} = 167 a t 1073 K

R = 0.0831 b a r L m o l^{- 1} K^{- 1}

K_{p}

K_{c}

K_{C}

K_{P}

2 N O C l (g) ⇌ 2 N O (g) + C l_{2} (g); K_{P} = 1.8 \times 10^{- 2}

500

C a C O_{3} (s) ⇌ C a O (s) + C O_{2} (g); K_{P} = 167

1073

= k [N O]^{2} [C l_{2}]

2 N O + C l_{2} \to 2 N O C l

2 N O + C l_{2} \to 2 N O C l

Rate = k [N O]^{2} [C l_{2}]

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