When 0.40 moles of SO2 and 0.60 moles of O2 are placed in an evacuated 1.00-liter flask, the reaction represented above occurs After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 moles of SO3. Based on these results, the value for the equilibrium constant, Kg of the reaction is... ○ 6.67 O 1.25 ○ 0.9375 02 ○ 4.62 0

Kc of the reaction is 0.9375

Explanation:

Step 1: Data given

Moles of SO2 = 0.40 moles

Moles of O2 = 0.60 moles

Volume = 1.00 L

After the reactio we find 0.30 moles SO3

Step 2: The balanced equation

2 SO2(g) + O2(g)  ⇔ 2SO3(g)

Step 3: Calculate Kc

Kc = [SO3]² / ([SO2]²[O2])

Kc = 0.30² / (0.40²*0.60)

Kc = 0.9375

Kc of the reaction is 0.9375

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