Imagine that a chemist puts 9.53 mol each of C2H2 and O2 in a 1.00-L container at constant temperature of 128 °C. This r...

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Imagine that a chemist puts 9.53 mol each of C2H2 and O2 in a 1.00-L container at constant temperature of 128 °C. This r...

Imagine that a chemist puts 9.53 mol each of C₂H₂ and O₂ in a 1.00-L container at constant temperature of 128 °C. This reaction occurs:

2C₂H₂(g) + 5O₂(g) ⇄ 4CO₂(g) + 2H₂O(g)

When equilibrium is reached, 1.71 mol of CO₂ is in the container. Find the value of K_eq for the reaction.

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Answer 1

Answer #1

Answer: K_eq = 3.76×10^-6

+4x +2x 2GH2(g) + 502(g) = 460,69) + 2H20 (9) Initial : 9.53 9.53 o o Change: -2x -sa +42 +22 Equilibrium! 9.53-28 9.53-50 4x

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Answer 2

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Imagine that a chemist puts 9.53 mol each of C2H2 and O2 in a 1.00-L container at constant temperature of 128 °C. This r...

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