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.
Here, we are going to calculate the empirical formula of the given oxide.
Empirical formula gives the simplest ratio of elements in a compound.
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.
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
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.