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Standard XII

Chemistry

Addition of Inert Gas at Constant Pressure

For the react...

Question

For the reaction: $C O (g) + 2 H_{2} (g) ⇌ C H_{3} O H (g)$ , find the equilibrium constant $K_{p}$ if $K_{c} = 2500$ at temperature 600 K?

4.92

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2.04

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1.03

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None of the above

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Solution

The correct option is C 1.03
We know that,
$K_{p} = K_{c} (R T)^{Δ n}$
$C O (g) + 2 H_{2} (g) ⇌ C H_{3} O H (g)$
for the given reaction $Δ n = 1 - 3 = - 2$
or $K_{p} = 2500 (0.082 \times 600)^{- 2}$
$K_{p} = 1.0327$

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Similar questions

{C H}_{3} O H (g)

can be prepared using equation,

C O (g) + 2 H_{2} (g) ⇌ {C H}_{2} O H (g),

K_{c} = {4 \times 10}^{2}

At equilibrium, a 5 L flask contains equal moles of

C O (g)

and

{C H}_{3} O H (g)

. Hence, number of moles of

H_{2}

at equilibrium is:

Q. For the reaction,

C O (g) + 2 H_{2} (g) ⇋ {C H}_{3} O H (g)

, hydrogen gas is introduced into a

5 L

flask at

327^{o} C

, containing

0.2

mole of

C O (g)

and a catalyst (solid), until the pressure is

4.92

atmosphere. At this point,

0.1

mole of

{C H}_{3} O H (g)

is formed. Calculate the equilibrium constants

K_{p}

and

K_{c}

The equilibrium constant for the reaction

H_{2 (g)} + C l_{2 (g)} \Leftrightarrow 2 H C l_{(g)}

K p

, at the given temperature. Find out the equilibrium constant for the reaction

H C l_{(g)} \Leftrightarrow \frac{1}{2} H_{2 (g)} + \frac{1}{2} C l_{2}

Q. The equilibrium constant

K_{c}

for the reaction,

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

0.08

at a certain temperature. If the equilibrium concentration of

C O C l_{2}

0.10 M

, what are the equilibrium concentration of

C O

and

C l_{2}

Q. In reaction

C O (g) + {2 H}_{2} (g) ⇄ {C H}_{3} O H (g); Δ_{f} H^{o} = - 92.0 k J / m o l

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Addition of Inert Gas at Constant Pressure

Standard XII Chemistry

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For the reaction: CO(g)+2H2(g)⇌CH3OH(g), find the equilibrium constant Kp if Kc=2500 at temperature 600 K?

The correct option is C 1.03We know that, Kp=Kc(RT)Δn CO(g)+2H2(g)⇌CH3OH(g) for the given reaction Δn=1−3=−2 or Kp=2500(0.082×600)−2 Kp=1.0327

For the reaction: $C O (g) + 2 H_{2} (g) ⇌ C H_{3} O H (g)$ , find the equilibrium constant $K_{p}$ if $K_{c} = 2500$ at temperature 600 K?

The correct option is C 1.03
We know that,
$K_{p} = K_{c} (R T)^{Δ n}$
$C O (g) + 2 H_{2} (g) ⇌ C H_{3} O H (g)$
for the given reaction $Δ n = 1 - 3 = - 2$
or $K_{p} = 2500 (0.082 \times 600)^{- 2}$
$K_{p} = 1.0327$