   # f 10.0 g of hydrogen gas is reacted with 10.0 g of oxygen gas according to the equation :math&gt; 2 H 2 + O 2 → 2 H 2 O should not expect to form 20.0 g of water. Why not? What mass of water can be produced with a complete reaction? ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425
Chapter 9, Problem 6ALQ
Textbook Problem
362 views

## f 10.0 g of hydrogen gas is reacted with 10.0 g of oxygen gas according to the equation:math> 2 H 2 + O 2 → 2 H 2 O should not expect to form 20.0 g of water. Why not? What mass of water can be produced with a complete reaction?

Interpretation Introduction

Interpretation:

Why 10 g of hydrogen gas when reacted with 10 g of oxygen gas, not give 20 g of water should be explained and the mass of water produced with a complete reaction should be determined.

Concept Introduction:

The amount of product obtained in a reaction depends on the amount of limiting reactant in the reaction. Limiting reactant is the reactant that completely consumes in the chemical reaction. The amount of product formed can be calculated from its number of moles which can be calculated by comparing the number of moles of limiting reactant in a balanced chemical reaction.

### Explanation of Solution

10 gram of hydrogen on reaction with 10 g of oxygen gas cannot gives 20 g of water because amount of water obtained depends on the amount of limiting reactant. To determine the limiting reactant, mass of oxygen obtained from both the reactants should be compared. The reactant that forms lesser amount of water is limiting reactant.

The balanced chemical reaction is as follows:

2H2+O22H2O

From the above chemical reaction, 2 moles of hydrogen gas reacts with 1 mole of oxygen gives 2 moles of water.

To calculate the mass of water, first calculate the number of moles of hydrogen and oxygen gas as follows:

n=mM

Here, m is mass and M is molar mass

For hydrogen gas: molar mass is 2 g/mol thus,

n=102=5 mol

Similarly, for oxygen: molar mass is 32 g/mol thus,

n=1032=0

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