Problem: A 1.00-L flask was filled with 2.00 moles of gaseous SO 2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.30 moles of gaseous NO was present. Assume that the reactionSO2(g) + NO2(g) ⇌ SO3(g) + NO(g)occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction.

🤓 Based on our data, we think this question is relevant for Professor Goldberg's class at Adelphi University.

FREE Expert Solution

Given reaction:SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)


Kc is an equilibrium expression:

Kc=productsreactants=[SO3][NO][SO2][NO2]

only gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression


  • molarity = mol/L


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Problem Details

A 1.00-L flask was filled with 2.00 moles of gaseous SO 2 and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, it was found that 1.30 moles of gaseous NO was present. Assume that the reaction

SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction.

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Based on our data, we think this problem is relevant for Professor Goldberg's class at Adelphi University.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.