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![PRACTICE PROBLEM 19-1: A reaction that is used in the production of sulfuric acid can be described by the chemical equation 2502(g) + O2(g) 늑 2SO3(g) If initially [SO,lo - 8.500 M, [Ol, 3.500 M, and [SO 5.575 M, and if [o,]-0.075 M at equilibrium, then calculate the equilibrium values of [SO2] and [So,].](https://media.cheggcdn.com/media%2Fa75%2Fa751eb3a-c3ff-45ea-ab34-5a087b182c33%2Fimage "Question & Answer: A reaction that is used in the production of sulphuric acid can be described by the chemical..... 1")
A reaction that is used in the production of sulphuric acid can be described by the chemical equation 2SO_2(g) + O_2(g) 2SO_3(g) If initially [SO_2]_0 = 8.500 M, [O_2]_0 = 3.500 M, and [SO_3]_0 = 5.575 M, and if [O_2] = 0.075 M at equilibrium, then calculate the equilibrium values of [SO_2] and [So_3].
Expert Answer
Answer
Since the concentration of O2 is going to be lower at equilibrium, the equilibrium must shift to the right.
2SO2 + O2 <–> 2SO3
I 8.5M 3.5M 5.575M
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C -2x -x +2x
E 8.5 -2x 3.5 – x 5.575 + 2x
Since the equilibrium of O2 is given, we can solve for x:
3.5-x=0.075
x=3.425
Plug this value into the equilibrium concentrations of So2 and So3:
[so2]= 8.5 – 2(3.425)
= 1.65M
[S03]=5.575 + 2(3.425)
=12.425M
