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Consider the following equilibrium: CO2(g) + H2(g)---CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose...

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Chemistry

Consider the following equilibrium: CO2(g) + H2(g)---CO(g) +H2O(g); Kc = 1.6 at 1260 K Suppose 0.038 mol CO2 and 0.022 mol H2are placed in a 1.50-L vessel at 1260 K. What is the equilibriumpartial pressure of CO(g)?

The answer is either 9.9 atm or 1.1 atm. But my question isWHY IS ONE CHOICE INCORRECT since I get both in mycalculations.

Answer & Explanation Solved by verified expert
4.5 Ratings (919 Votes)
KC 16 K COH2O CO2H2 T 1260 CO2 nV 003815 00253 M H2 002215 001466666 M CO 0 H2O in equilibrium CO2 00253 x H2 001466666 x CO 0 x H2O 0 x substitute in K K COH2O CO2H2 16 xx00253    See Answer
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