at equilibrium in a 10L vessel, there are 7.60x10^-2 moles of SO2, 8.60x10^-2 moles of O2,...

at equilibrium in a 10L vessel, there are 7.60x10^-2 moles of SO2, 8.60x10^-2 moles of O2, and 8.20x10^-2 moles of SO3. What is the equilibrium constant Kc under these conditions for the following reaction?

2SO2(g) + O2(g) -> 2SO3 (g)

a) 135

b) 12.5

c) 13.5

d) 125

Expert Solution

Steps to calculate the Equilibrium constant of a given reaction:

1. Calculate the concentration of each component of the reaction at equilibrium. We also call this concentration as 'Equilibrium concentration'. In this question, we were given the equilibrium moles of each component and also the volume of the container. Hence we calculated the equilibrium concentration by dividing the equilibrium moles of each component by the volume of the container.

Important point to note:

While calculating the equilibrium constant, we only take into account the gaseous components. Pure solid and liquid are not used in the calculations Since they don't affect the equilibrium.Since, in this particular question all the components were in gaseous state we took all of them into account while calculating the Kc.(Equilibrium constant).

2. Next the Equilibrium formula is used to directly calculate the Equilibrium constant.

Hence, the answer is a) 135.

queen_honey_blossom answered 2 years ago

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