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K(c ) for CO(g)+H(2)O(g) hArr CO(2)(g)+H...

`K_(c )` for `CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g)` at `986^(@)C` is `0.63`. A mixture of `1` mol `H_(2)O(g)` and `3` mol `CO (g)` is allowed to react to come to an equilibrium. The equilibrium pressure is `2.0` atm.
a. How many moles of `H_(2)` are present at equilibrium ?
b. Calculate partial pressure of each gas at equilibrium.

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To solve the problem step by step, we will analyze the given reaction and the equilibrium conditions. ### Given Reaction: \[ \text{CO(g)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO}_2(g) + \text{H}_2(g) \] ### Given Data: - \( K_c = 0.63 \) at \( 986^\circ C \) - Initial moles of \( \text{H}_2\text{O} = 1 \, \text{mol} \) ...
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