A compound is found to contain 3.1% Hydrogen, 65.3% Oxygen and 31.6% Phosphorus. Work out its empirical formula.

To answer this question, we need to know the relative number of atoms of each element present. This can be calculated by dividing the amount of an element present in the sample by the relative masses of that element. Relative masses: Hydrogen = 1.0 Oxygen = 16.0 Phosphorus = 30.0. Relative number of atoms = (%composition)/(relative atomic mass) Hydrogen = 3.1 Oxygen = 4.08 Phosphorus = 1.05. This gives us the relative ratios of the elements: 3H's, 4O's, 1P. Therefore the empirical formula is H3PO4.

AB
Answered by Adam B. Chemistry tutor

5219 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

Name or formulate these compounds: i)CH3CH2CH(CH3)COOH ii)CH3CH2COCH3 iii) 3-hydroxy-2-pentanone iv) 1-propanamine


What are Oxidation and Reduction?


What determines rate of reaction?


A student wishes to investigate the effect of surface area on the rate of reaction between marble chips and hydrochloric acid. Which variables should he control?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences