Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
The following equilibrium exists at 637 K.rn2 SO3(g) equilibrium reaction arrow 2 SO2(g) + O2(g); rnkp = 2.10 ✕ 10−5rn(a) Calculate kc for this reaction.
Accepted Answer
Calculate the equilibrium constant Kc from the equilibrium constant Kp using the following equation:
Kc=Kp/(RT)^Δn
where:
R is the ideal gas constant (0.0821 Latm/(molK))
T is the temperature in Kelvin (637 K)
Δn is the change in the number of moles of gas in the balanced chemical equation
For the given reaction:
2 SO3(g) ⇌ 2 SO2(g) + O2(g)
Δn = (2 + 1) - 2 = 1
Substitute the values into the equation:
Kc=(2.10×10−5)/(0.0821×637)^1
Kc=6.25×10−3
Therefore, the equilibrium constant Kc for the reaction is 6.25×10−3.
Articles you might like