Show Summary Details
Making the Transition to University Chemistry

Making the Transition to University Chemistry

Michael Clugston, Malcolm Stewart, and Fabrice Birembaut
Page of

Printed from Oxford Science Trove. Under the terms of the licence agreement, an individual user may print out a single article for personal use (for details see Privacy Policy and Legal Notice).

date: 17 June 2024

p. 26 Chapter 3 Moleslocked

p. 26 Chapter 3 Moleslocked

  • Michael Clugston, Michael Clugstonformerly Tonbridge School
  • Malcolm StewartMalcolm StewartUniversity of Oxford
  •  and Fabrice BirembautFabrice BirembautCaen, France

Abstract

This chapter explores different types of formulae in chemistry: empirical formula and molecular formula. It defines empirical formula as the simplest whole-number ratio of atoms of each element in a compound. Molecular formula can be defined as the whole-number multiple of the empirical formula. The chapter also explains the value of the Avogadro constant, which is the number of atoms per mole. It notes the strategies for solving mass-to-mass calculations, ideal gas models, molar concentration, and molar volume. Molar mass is defined as the mass per mole of a substance. A solution is mostly expressed through mass concentration. This specifies the mass of the solute dissolved per cubic decimetre of the solution.

You do not currently have access to this article

Login

Please login to access the full content.

Subscribe

Access to the full content requires a subscription