\( \mathrm{K}_{\mathrm{P}} \) for the reaction: \( \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\....

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\( \mathrm{K}_{\mathrm{P}} \) for the reaction:
\( \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \) is found to be
\( \mathrm{P} \)
16 at a given temperature. Originally equal number of moles of \( \mathrm{H}_{2} \) and \( \mathrm{CO}_{2} \) were placed in the flask. At equilibrium, the pressure of \( \mathrm{H}_{2} \) is \( 1.20 \mathrm{~atm} \). What is the partial pressure of \( \mathrm{CO} \) ?
(1) \( 1.20 \mathrm{~atm} \)
(2) \( 2.40 \mathrm{~atm} \)
(3) \( 4.80 \mathrm{~atm} \)
(4) \( 9.60 \mathrm{~atm} \)


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