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?1(DELL O$300 9634368ABUSES

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?.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 91AP: Consider the following reaction: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) a container were to have only 10...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

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?
1
(DELL O
$300 9634368
ABUSES

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