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ANALYZING DATA A chemical engineer calculated that 15.0
Chapter 9, Problem 9.1.13(choose chapter or problem)
ANALYZING DATA A chemical engineer calculated that 15.0 mol H2 was needed to react with excess N2 to prepare 10.0 mol NH3. But the actual yield is 60.0%. Write a balanced chemical equation for the reaction. Is the amount of H2 needed to make 10.0 mol NH3 more than, the same as, or less than 15 mol? How many moles of H2 are needed?
Questions & Answers
QUESTION:
ANALYZING DATA A chemical engineer calculated that 15.0 mol H2 was needed to react with excess N2 to prepare 10.0 mol NH3. But the actual yield is 60.0%. Write a balanced chemical equation for the reaction. Is the amount of H2 needed to make 10.0 mol NH3 more than, the same as, or less than 15 mol? How many moles of H2 are needed?
ANSWER:Step 1 of 3
The moles of hydrogen needed = 15 moles
The actual number of moles that are present is 60% and are only 9 moles.
These are less than 15, that is the required number of moles.