Consider the following reaction at STP: 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g) How many moles of S will form when 9.2 moles of H2S reacts with 4.8 moles of SO2? Identify the limiting reagent: Identify the excess reagent: How many moles of the excess reagent will remain after the reaction is finished?
Consider the following reaction at STP: 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g) How many moles of S will form when 9.2 moles of H2S reacts with 4.8 moles of SO2? Identify the limiting reagent: Identify the excess reagent: How many moles of the excess reagent will remain after the reaction is finished?
Chemistry: Principles and Reactions
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Author:William L. Masterton, Cecile N. Hurley
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Chapter8: Thermochemistry
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Consider the following reaction at STP: 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g)
How many moles of S will form when 9.2 moles of H2S reacts with 4.8 moles of SO2?
Identify the limiting reagent: Identify the excess reagent:
How many moles of the excess reagent will remain after the reaction is finished?
Expert Solution
Step 1
Considering the given reaction:
2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O (g)
2 mol 1 mol 3 mol 2 mol
According to the reaction:
2 mol of H2S react with 1 mol of SO2
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