Soo, my chemistry teacher couldn't even help me with this...
One of the reactions used to form sulfuric acid is the reaction of oxygen with sulfur dioxide under equilibrium conditions to form sulfur trioxide.
Before the reaction, the concentration of sulfur dioxide was 0.006 molL-1 and the concentration of oxygen was 0.05 molL-1. After the equilibrium was reached, the concentration of sulfur trioxide was 0.04 molL-1
Calculate the equilibrium constant , K, for the reaction. Show relevant working.
The back of the book says the answer is...
K = [0.04]^2 / [0.02]^2 x [0.03]
= 133
But I get...
K = [0.04]^2 / [0.06]^2 x [0.05]
I'm not sure how to get the correct answer. Would anyone mind walking me through the process?
One of the reactions used to form sulfuric acid is the reaction of oxygen with sulfur dioxide under equilibrium conditions to form sulfur trioxide.
Before the reaction, the concentration of sulfur dioxide was 0.006 molL-1 and the concentration of oxygen was 0.05 molL-1. After the equilibrium was reached, the concentration of sulfur trioxide was 0.04 molL-1
Calculate the equilibrium constant , K, for the reaction. Show relevant working.
The back of the book says the answer is...
K = [0.04]^2 / [0.02]^2 x [0.03]
= 133
But I get...
K = [0.04]^2 / [0.06]^2 x [0.05]
I'm not sure how to get the correct answer. Would anyone mind walking me through the process?