   Chapter 2, Problem 112GQ

Chapter
Section
Textbook Problem

When a sample of phosphorus burns in air, the compound P4O10 forms. One experiment showed that 0.744 g of phosphorus formed 1.704 g of P4O10. Use this information to determine the ratio of the atomic weights of phosphorus and oxygen (mass P/mass O). If the atomic weight of oxygen is assumed to be 16.000, calculate the atomic weight of phosphorus.

Interpretation Introduction

Interpretation:

The ratio of atomic weights of phosphorus and oxygen and the atomic weight of phosphorus are needed to be calculated.

Concept introduction:

Mass of a compound is the sum of the mass of all the atoms present in the compound.

Explanation

The mass of phosphorus and P4O10 in the experiment are given as 0.744g and 1.704g respectively.

Therefore,

The mass of oxygen present in the P4O10 is,

1.704g0.744g=0.96g

There are 4P and 100 atoms in P4O10, the mass of 4P and 6O atoms are 0

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

What are the chemical differences between DNA and RNA?

Biology: The Dynamic Science (MindTap Course List)

Match the term listed in Column A with its definition from Column B

Nutrition Through the Life Cycle (MindTap Course List)

How is pH expressed?

Oceanography: An Invitation To Marine Science, Loose-leaf Versin 