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625) mixture of 3.8 moles of NO and 0.92 CO2 was allowed to react in a 1.0 L co e equilibrium mixture contains 0.124 2. Calculate Kc for the reaction Die + CO2(g) NO2(g) + CO

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Similar Questions

A mixture of 3.8 moles of NO and 0.924 moles of

C O_{2}

was allowed to react in a 1.0 L container.The equilibrium mixture contains 0.124 mole of

C O_{2}

.Calculate

K_{c}

for the reaction.

N O_{(g)} + C O_{2 (g)} ⇌ N O_{2 (g)} + C O_{(g)}

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The equilibrium constant for the reaction,

C O (g) + H_{2} O (g) ⇌ C O_{2} (g) + H_{2} (g)

986^{o} C

0.63

. A mixture of

1.0

mole of water vapor and

3.0

moles of

C O

is allowed to come to equilibrium. The equilibrium pressure is

2.0 a t m

(i) How many moles of

H_{2}

are present at equilibrium?
(ii) Calculate the partial pressure of gases in the equilibrium mixture.

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In an experiment,

o n e m o l e

of acetic acid and

o n e m o l e

of alcohol were allowed to react until equilibrium was established. The equilibrium mixture was found to contain

2 / 3 m o l e

of the ester. Calculate the equilibrium constant of the reaction.

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The equilibrium constant for the following reaction:
$$CO(g)+H_2O(g)\rightleftharpoons CO_2(g)+H_2(g)$$
at $$986^oC$$ is $$0.63$$. A mixture of $$1.0$$ mole of water vapour and $$3.0$$ mole of CO is allowed to come to equilibrium. The equilibrium pressure is $$2.0$$ atm.
Calculate the partial pressures of gases in the equilibrium mixture.

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1127 K

and

1 a t m

pressure, a gaseous mixture of

C O

and

C O_{2}

in equilibrium with solid carbon has

90.55

C O

by mass

C (s) + C O_{2} (g) ⇋ 2 C O (g)

Calculate

K_{c}

for this reaction at the above temperature.

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