   Chapter 1, Problem 13PS

Chapter
Section
Textbook Problem

An 18 g sample of water is decomposed into 2 g of hydrogen gas and 16 g of oxygen gas. What masses of hydrogen and oxygen gases would have been prepared from 27 g of water? What law of chemistry is used in solving this problem?

Interpretation Introduction

Interpretation:

The amount of hydrogen and oxygen gas produced in the decomposition reaction and the law of chemistry used to calculate the masses has to be given.

Concept introduction:

Law of definite proportion: A given compound always contains its component elements in fixed ratio (by mass) and does not depend on its source and method of preparation.

Explanation

Given,

Mass of water = 18g

Mass of oxygen = 16g

Mass of hydrogen = 2g

The amount of hydrogen and oxygen produced is calculated as,

Amount of H2produced:_18g of H2O produces 2g of H2 gas,Therefore,27g of H2O produces (x)g of H2 gas,Hence, x = (27)(2)18 = 3gof H2 gas

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