laboratory experiment, 20.0 g of Cu were reacted with 90.0 g HNO3. 3 Cu + 8 HNO3 3 Cu(NO3)2 + 4 H2O + 2 NO (a) Calculate in grams the mass of Cu(NO3)2 that can be theoretically produced? (b) Based on your answer in 4(a) which reactant is the limiting reactant and which reactant is in excess? (c) When 20.0 g of Cu reacts with 90.0 g HNO3, and 40.5 g of Cu(NO3)2 is recovered, what is the percent yield of Cu(NO3)2?
laboratory experiment, 20.0 g of Cu were reacted with 90.0 g HNO3. 3 Cu + 8 HNO3 3 Cu(NO3)2 + 4 H2O + 2 NO (a) Calculate in grams the mass of Cu(NO3)2 that can be theoretically produced? (b) Based on your answer in 4(a) which reactant is the limiting reactant and which reactant is in excess? (c) When 20.0 g of Cu reacts with 90.0 g HNO3, and 40.5 g of Cu(NO3)2 is recovered, what is the percent yield of Cu(NO3)2?
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.44PAE: 4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of...
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In a laboratory experiment, 20.0 g of Cu were reacted with 90.0 g HNO3.
3 Cu + 8 HNO3 3 Cu(NO3)2 + 4 H2O + 2 NO
(a) Calculate in grams the mass of Cu(NO3)2 that can be theoretically produced?
(b) Based on your answer in 4(a) which reactant is the limiting reactant and which
reactant is in excess?
(c) When 20.0 g of Cu reacts with 90.0 g HNO3, and 40.5 g of Cu(NO3)2 is recovered,
what is the percent yield of Cu(NO3)2?
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