At `1127 K` and `1 atm` pressure, a gaseous mixture of `CO` and `CO_(2)` in equilibrium with solid carbon has `90.55% CO` by mass:
`C_((s))+CO_(2(s))hArr2CO_((g))`
Calculate `K_(c)` for the reaction at the above temperature.

Explanation

To find the equilibrium constant \( K_c \) for the reaction

\[ C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)} \]

at a temperature of \( 1127 \, K \) and \( 1 \, atm \) pressure, we can follow these steps:

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