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Activation Energy

The equilibri...

Question

The equilibrium constant kp for the reaction H2g) + CO2,g) gives H2O(g) CO(g) is 4.0 at 1660^° C. Initially0.80 mole H2, and 0.80 mole CO2 are injected into a 5.0 liter flask. What is the equilibrium concentration of co2

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Q. The equilibrium constant

K_{P}

for the reaction

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

4.0

1660^{\circ} C

0.80 m o l e H_{2}

0.80 m o l e C O_{2}

are injected into a

5.0 l i t r e

flask. What is the equilibrium concentration of

C O_{2} (g)

?

Q. At a given temperature,

K c

4

for the reaction :

H_{2 (g)} + C {O_{2}}_{(g)} \Leftrightarrow H_{2} O_{(g)} + C O_{(g)}

0.6

H_{2}

C O_{2}

1

liter flask. The equilibrium concentration of

H_{2} O_{(g)}

Q. The equilibrium constant for,

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

1.80

1000^{o}

1.0

H_{2}

1.0

C O_{2}

are placed in one litre flask, the final equilibrium concentration of

C O

1000^{o}

675 K

H_{2} (g)

C O_{2} (g)

C O (g)

H_{2} O (g), K_{p}

for the reaction is

0.16

. If a mixture of

0.25

H_{2}

0.25

C O_{2}

675 K

, mole percentage of

C O (g)

in equilibrium mixture is:

Q. The equilibrium constant for the reaction

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

at a certain temperature is

2.2

. Initially one mole of CO and one mole of

H_{2} O

are placed in a

2.0

L container. What are the concentrations of all the substances when the reaction reached equilibrium?

([C O_{2}] = [H_{2}] = 0.2986 M, [C O] = [H_{2} O] = 0.2014 M)

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