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A 1.45-g sample of phosphorus burns in air and forms 2.57

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 95P Chapter 6

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 95P

A 1.45-g sample of phosphorus burns in air and forms 2.57 g of a phosphorus oxide. Calculate the empirical formula of the oxide.

Step-by-Step Solution:

Solution  95P

Here, we are going to calculate the empirical formula of the given oxide.

Step 1:

Empirical formula gives the simplest ratio of elements in a compound.

Step 2:

Given, total mass of phosphorus oxide formed = 2.57 g

        Mass of phosphorus sample used = 1.45 g

Therefore, mass of oxygen in phosphorus oxide = 2.57 g - 1.45 g = 1.12 g

Now, let us calculate the empirical formula using the above data.

Step 3 of 3

Chapter 6, Problem 95P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: oxide, phosphorus, forms, empirical, calculate. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Since the solution to 95P from 6 chapter was answered, more than 1032 students have viewed the full step-by-step answer. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The answer to “A 1.45-g sample of phosphorus burns in air and forms 2.57 g of a phosphorus oxide. Calculate the empirical formula of the oxide.” is broken down into a number of easy to follow steps, and 23 words. The full step-by-step solution to problem: 95P from chapter: 6 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.

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