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Byju's Answer

Standard XII

Chemistry

Elevation in Boiling Point

At 1127 K and...

Question

At 1127 K and 1 atm pressure, a gaseous mixture of CO and CO₂ in equilibrium with solid carbon has 90.55% CO by mass

Calculate K_c for this reaction at the above temperature.

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Solution

Let the total mass of the gaseous mixture be 100 g.

Mass of CO = 90.55 g

And, mass of CO₂ = (100 – 90.55) = 9.45 g

Now, number of moles of CO,

Number of moles of CO₂,

Partial pressure of CO,

Partial pressure of CO₂,

For the given reaction,

Δn = 2 – 1 = 1

We know that,

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Similar questions

At 1127 K and 1 atm pressure, a gaseous mixture of CO and $C O_{2}$ in equilibrium with solid carbon has 90.55% CO by mass
$C (s) + C O_{2} (g) \leftrightarrow 2 C O (g)$
Calculate $K_{c}$ for this reaction at the above temperature.

Q. At

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.

Q. At

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 the reaction at the above temperature.

Q. At

1127

K and

1

atm pressure, a gaseous mixture of CO and

C O_{2}

in equilibrium with solid carbon has

90.55 %

CO by mass,

C_{(s)} + C O_{2 (g)} ⇌ 2 C O_{(g)}

K_{c}

for this reaction at the above temperature is:

Q. At high temperature of

727^{\circ} C

a dynamic equilibrium exists between

C O, C O_{2}

and solid carbon.

C (s) + C O_{2} (g) ⇌ 2 C O (g)

;

K_{c} = 0.1 M

Then value of

K_{p}

at given temperature is:

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At 1127 K and 1 atm pressure, a gaseous mixture of CO and CO2 in equilibrium with solid carbon has 90.55% CO by mass Calculate Kc for this reaction at the above temperature.

Let the total mass of the gaseous mixture be 100 g. Mass of CO = 90.55 g And, mass of CO2 = (100 – 90.55) = 9.45 g Now, number of moles of CO, Number of moles of CO­2, Partial pressure of CO, Partial pressure of CO2, For the given reaction, Δn = 2 – 1 = 1 We know that,

At 1127 K and 1 atm pressure, a gaseous mixture of CO and CO₂ in equilibrium with solid carbon has 90.55% CO by mass

Calculate K_c for this reaction at the above temperature.

Let the total mass of the gaseous mixture be 100 g.

Mass of CO = 90.55 g

And, mass of CO₂ = (100 – 90.55) = 9.45 g

Now, number of moles of CO,

Number of moles of CO₂,

Partial pressure of CO,

Partial pressure of CO₂,

For the given reaction,

Δn = 2 – 1 = 1

We know that,