# 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.

###### FREE Expert Solution

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

Kc is an equilibrium expression:

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}{\mathbf{=}}\frac{\mathbf{\left[}{\mathbf{SO}}_{\mathbf{3}}\mathbf{\right]}\mathbf{\left[}\mathbf{NO}\mathbf{\right]}}{\mathbf{\left[}{\mathbf{SO}}_{\mathbf{2}}\mathbf{\right]}\mathbf{\left[}{\mathbf{NO}}_{\mathbf{2}}\mathbf{\right]}}}$

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.