The value of Kp for the reaction, 2H2S(g)2H2(g)+S2(g) is 1.2× 10-2 1065oC. The value for Kc is

Question

The value of Kp for the reaction, 2H2S(g)2H2(g)+S2(g) is 1.2× 10-2 1065oC. The value for Kc is (A)  <1.2× 10-2  (B)  >1.2× 10-2  (C)  1.2× 10-2  (D)  0.12× 10-2

Tardigrade Admin · Accepted Answer

Δ ng= moles of gaseous products - moles of gaseous reactants, = 3 ? 2 ? 1 = 0 Kp=Kc(RT)Δ ng Kc=(Kp/RT) =(1.2× 10-2/0.0821× 1338) =1.09× 10-4<1.2× 10-2

Q. The value of $K_{p}$ for the reaction, $2 H_{2} S (g) 2 H_{2} (g) + S_{2} (g)$ is $1.2 \times 10^{- 2}$ $1065^{o} C .$ The value for $K_{c}$ is

$< 1.2 \times 10^{- 2}$

$> 1.2 \times 10^{- 2}$

$1.2 \times 10^{- 2}$

$0.12 \times 10^{- 2}$

$Δ n_{g} =$ moles of gaseous products - moles of gaseous reactants, = 3 ? 2 ? 1 = 0 $K_{p} = K_{c} (RT)^{Δ n_{g}}$ $K_{c} = \frac{K _{p}}{RT}$ $= \frac{1.2 \times 10 ^{- 2}}{0.0821 \times 1338}$ $= 1.09 \times 10^{- 4} < 1.2 \times 10^{- 2}$

Q. The value of Kp​ for the reaction, 2H2​S(g)2H2​(g)+S2​(g) is 1.2×10−2 1065oC. The value for Kc​ is

<1.2×10−2

>1.2×10−2

1.2×10−2

0.12×10−2