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Standard XIII

Chemistry

Relation between Kp and Kc

Kp for a reac...

Question

$K_{p}$ for a reaction at $25^{o} C$ in 10 atm is 8.568. Then $K_{c}$ for the reaction at $25^{o} C$ will be:
$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$

4.33 \times 10^{- 1} M

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3.33 \times 10^{- 2} M

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3.89 \times 10^{- 1} M

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none of these

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Solution

The correct option is D none of these
We know, relation between the reactions constants as:
$K_{p} = K_{c} (R T)^{△ n},$
As per reaction:
$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$ $△ n = - 2$
$∴ 8.568 \times (0.0821 \times 313)^{2} = K_{c}$
$K_{c} \Rightarrow 5657.88$

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Similar questions

K_{p}

for a reaction at

25^{o} C

in 10 atm is 8.568. Then

K_{c}

for the reaction at

25^{o} C

will be:

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

Δ G^{o}

for

\frac{1}{2} N_{2} (g) + \frac{3}{2} H_{2} (g) ⇌ {N H}_{3} (g)

- 16.5 k J {m o l}^{- 1}

. Find out

K_{p}

for the reaction at

25^{o} C

. Also report

K_{p}

and

Δ G^{o}

for

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)

25^{o} C

Q. The equilibrium constant

K_{c}

for the reaction

N_{2 (g)} + 3 H_{2} ⇌ {2 N H}_{3 (g)}

0.286

500^{o} C

. Calculate

K_{c}

and

K_{p}

for the reaction

2 N H_{3 (g)} ⇌ N_{2 (g)} + {3 H}_{2 (g)}

K_{p}

for the reaction

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)

, at

298 K

5.2 \times 10^{- 5}

. What is the value of

K_{c}

298 K

, for the reaction

\frac{1}{2} N_{2} (g) + \frac{3}{2} H_{2} (g) ⇌ {N H}_{3} (g)

K_{p}

for a reaction at

25^{o} C

in 10 atm is 8.568. Then

K_{c}

for the reaction at

25^{o} C

will be:

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

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Relation between Kp and Kc

Standard XIII Chemistry

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Kp for a reaction at 25oC in 10 atm is 8.568. Then Kc for the reaction at 25oC will be: N2(g)+3H2(g)→2NH3(g)

The correct option is D none of these We know, relation between the reactions constants as: Kp=Kc(RT)△n, As per reaction: N2(g)+3H2(g)→2NH3(g) △n=−2 ∴8.568×(0.0821×313)2=Kc Kc⇒5657.88

$K_{p}$ for a reaction at $25^{o} C$ in 10 atm is 8.568. Then $K_{c}$ for the reaction at $25^{o} C$ will be:
$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$

The correct option is D none of these
We know, relation between the reactions constants as:
$K_{p} = K_{c} (R T)^{△ n},$
As per reaction:
$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$ $△ n = - 2$
$∴ 8.568 \times (0.0821 \times 313)^{2} = K_{c}$
$K_{c} \Rightarrow 5657.88$