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Standard XIII

Chemistry

Derivation of Kp and Kc

At 3000 K the...

Question

At 3000 K the equilibrium pressures of $C O_{2},$ CO and $O_{2}$ are 0.6, 0.4 and 0.2 atmospheres respectively. $K_{p}$ for the reaction, $2 C O_{2} ⇌ 2 C O + O_{2}$ is

0.089

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0.0533

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0.133

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0.177

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Solution

The correct option is A
0.089

$K_{p} = \frac{[p_{C O}]^{2} [p_{O_{2}}]}{[p_{C O_{2}}]^{2}} = \frac{[0.4]^{2} \times [0.2]}{[0.6]^{2}} = 0.0888$

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Similar questions

Q. At

3000 K

, the equilibrium partial pressure of

{C O}_{2}

C O

and

O_{2}

are

0.6, 0.4

and

0.2

atmospheres respective,y.

K_{p}

for the reaction,

2 C O_{2} (g) ⇌ 2 C O (g) + O_{2} (g)

is__________.

Q. If the equilibrium constant for reaction (i) is 2, what is the equilibrium constant for reaction (ii)?

C O_{2} ⇌ C O + \frac{1}{2} O_{2}

..... (i)

2 C O + O_{2} ⇌ 2 C O_{2}

.... (ii)

Q. For the reaction,

C (s) + C O_{2} (g) ⇌ 2 C O (g)

, the partial pressures of

C O_{2}

and

C O

are 2.0 and 4.0 atm respectively at equilibrium. The

K_{p}

for the reaction is:

Q. The dissociation of

C O_{2}

can be expressed as

2 C O_{2} ⇌ 2 C O + O_{2}

. If the 2 moles of

C O_{2}

is taken initially and 40% of the

C O_{2}

is dissociated equilibrium then total number of moles at equilibrium is:

C (s) + C O_{2} (g) ⇋ 2 C O (g)

For the given reaction, the partial pressures of

C O_{2}

and CO are 4.0 and 4.0 respectively at equilibrium, what is the value of

K_{p}

for this reaction?

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At 3000 K the equilibrium pressures of CO2, CO and O2 are 0.6, 0.4 and 0.2 atmospheres respectively. Kp for the reaction, 2CO2⇌2CO+O2 is

The correct option is A 0.089 Kp=[pCO]2[pO2][pCO2]2=[0.4]2×[0.2][0.6]2=0.0888

At 3000 K the equilibrium pressures of $C O_{2},$ CO and $O_{2}$ are 0.6, 0.4 and 0.2 atmospheres respectively. $K_{p}$ for the reaction, $2 C O_{2} ⇌ 2 C O + O_{2}$ is

The correct option is A
0.089

$K_{p} = \frac{[p_{C O}]^{2} [p_{O_{2}}]}{[p_{C O_{2}}]^{2}} = \frac{[0.4]^{2} \times [0.2]}{[0.6]^{2}} = 0.0888$