`0.20` mole of `CO` was taken in a `2.50` L flask maintained at `750` K along with a catalyst so that the following reac

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Q 1148512403.     `0.20` mole of `CO` was taken in a `2.50` L flask maintained at `750` K along with a catalyst so that the following reaction could take place:

`CO(g) + 2H_2(g) ⇌ CH_3OH(g)`

Hydrogen was introduced until the total pressure in the flask at equilibrium was `12.30` atm and `0.10` mole of `CH_3OH` was formed.

Find the equilibrium constant (in terms of `10^(-2)` `atm^(-2)`) of the reaction in terms of partial pressures.
A

`1.83`

B

`2.21`

C

`2.63`

D

`1.14`

HINT


Solution
(Provided By a Student and Checked/Corrected by EXXAMM.com Team)

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