# Chemistry Practice Problems## 5. Calculate:Suppose you had 2.0158 grams of hydrogen (H₂).A. How many moles of hydrogen do you have? ___________________B. How many moles of oxygen would react with this much hydrogen? ___________________C. What mass of oxygen would you need for this reaction? ___________________D. How many grams of water would you produce? ___________________## 6. Challenge Yourself:Suppose you wanted to make 100 grams of water.A. What is the molar mass of water (H₂O)? ___________________B. How many moles of water are in 100 grams? ___________________C. How many moles of hydrogen will you need? ___________________D. How many moles of oxygen will you need? ___________________E. How many grams of hydrogen and oxygen will you need? - Hydrogen: ___________________ - Oxygen: ___________________F. Is your answer reasonable? Why or why not? ___________________## 7. Summarize:Why is it useful to use moles to measure chemical quantities? ___________________ ___________________ ___________________

First we need to write a balanced chemical equation of hydrogen and oxygen to produce water. A.)…

5. Calculate: Suppose you had 2.0158 grams of hydrogen (H₂). A. How many moles of hydrogen do you have? B. How many moles of oxygen would react with this much hydrogen? C. What mass of oxygen would you need for this reaction? D. How many grams of water would you produce?.

5. Calculate: Suppose you had 2.0158 grams of hydrogen (H₂). A. How many moles of hydrogen do you have? B. How many moles of oxygen would react with this much hydrogen? C. What mass of oxygen would you need for this reaction? D. How many grams of water would you produce?.

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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