Lambert O'Quinn
03/18/2023 · Primary School
Use the References to access important values if needed for this question. The equilibrium constant in terms of pressures for the reduction of tungsten(IV) oxide to tungsten at \( 25^{\circ} \mathrm{C} \) is \( \mathrm{K}_{\mathrm{p}}=3.82 \times 10^{-4} \), corresponding to the reaction \[ \mathrm{WO}_{2}(\mathbf{s})+2 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{W}(\mathrm{s})+2 \mathrm{CO}_{2}(\mathrm{~g}) \] If the total pressure of an equilibrium system at \( 25^{\circ} \mathrm{C} \) is 2.33 atm , calculate the partial pressures of \( \mathrm{CO}(\mathrm{g}) \) and \( \mathrm{CO}_{2}(\mathrm{~g}) \).
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The partial pressures are \( P_{\mathrm{CO}} \approx 2.20 \, \text{atm} \) and \( P_{\mathrm{CO}_2} \approx 0.13 \, \text{atm} \).
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