How many moles of sulfur dioxide (SO2) are required to produce 5.0 moles of sulfur (S) according to the following balanced equat
2 answers:
Answer:
1.67 moles
Explanation:
From the balanced equation of reaction:
1 mole of sulfur dioxide, SO2, is required to produce 3 moles of sulfur, S.
<em>If 1 mole SO2 = 3 moles S, then, how many moles of SO2 would be required for 5 moles S?</em>
Moles of SO2 needed = 5 x 1/3
= 5/3 or 1.67 moles
Hence, <u>1.67 moles of SO2 would be required to produce 5.0 moles of S.</u>
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Answer: Concentration of in the equilibrium mixture is 0.31 M
Explanation:
Equilibrium concentration of = 0.729 M
The given balanced equilibrium reaction is,
Initial conc. x 0 0
At eqm. conc. (x-2y) M (y) M (3y) M
The expression for equilibrium constant for this reaction will be:
3y = 0.729 M
y = 0.243 M
Now put all the given values in this expression, we get :
concentration of in the equilibrium mixture =
Thus concentration of in the equilibrium mixture is 0.31 M