Consider the balanced equation:2 Na + H₂SO4 → Na2SO4+H₂1. If 35.0 g of Na is reacted with excess H₂SO4, what is the theoretical mass of H₂produced?2. If 1.1g of H₂ is actually produced, what is the percent yield of H₂?_Return to the balance with both

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Consider the balanced equation: 2 Na + H₂SO4 → Na2SO4+H₂ 1. If 35.0 g of Na is reacted with excess H₂SO4, what is the theoretical mass of H₂ produced? to moil ben mi. Neaker 2. If 1.1g of H₂ is actually produced, what is the percent yield of H₂?_

Consider the balanced equation: 2 Na + H₂SO4 → Na2SO4+H₂ 1. If 35.0 g of Na is reacted with excess H₂SO4, what is the theoretical mass of H₂ produced? to moil ben mi. Neaker 2. If 1.1g of H₂ is actually produced, what is the percent yield of H₂?_

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Consider the balanced equation:
2 Na + H₂SO4 → Na2SO4+H₂
1. If 35.0 g of Na is reacted with excess H₂SO4, what is the theoretical mass of H₂
produced?
2. If 1.1g of H₂ is actually produced, what is the percent yield of H₂?_
Return to the balance with both

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