Calculate the value of the equilibrium constant, kc, for the reaction below, if 0.208 moles of sulfur dioxide gas, 0.208 moles of oxygen gas and 0.425 moles of sulfur trioxide gas are present in a 1.50-liter reaction vessel at equilibrium.

2so2(g) +o2 (g) < --> 2so3 (g)

a. kc=3.32 x 10^-2
b. kc=2.01 x 10^1 (i know for a fact this one is wrong.)
c. kc=2.98 x 10^1
d. kc=1.47 x 10^1

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answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :