Get an answer in 5 minutes

We'll notify as soon as your question has been answered.

Plus iconAsk a question to our educators
CHEMISTRY
Asked by Bally

0.64 grams of copper when heated in air form 0.80grams of copper oxide. What is the simplest formula of copper oxide?

The moles of Cu reacted in excess oxygen is: mass / atomic mass of Cu = 0.01 mol. The moles of copper oxide formed will be some fraction (half, third, quarter, etc.) of 0.01 mol, depending on how the formula balances. Let’s call the big stochiometric coefficient in front of copper oxide ‘n’. The moles of copper oxide is therefore 0.01 x n, and the formula mass of copper oxide must be: mass / moles = 0.80 g / 0.01n = 80/n grams per mole. Remember, 64 g/mol of this 80 g/mol comes from a single Cu atom. The remaining 16 g/mol constitutes one O atom in each mole. So the simplest formula must be CuO, though Cu2O2, Cu3O3, etc. would result from using n values of 1/2, or 1/3, etc., rather than 1. This is what the question meant by ‘simplest formula’, because the others, while maintaining the correct molar ratio between Cu and O (1:1), do not accurately reflect the actual mass of the system (i.e. are multiples of the actual masses since there is an integer multiple of moles of the elements). I hope that helps!

Calem's profile picture
Verified
Calem Curreen
·

400 students helped

Similar Chemistry questions

Get an answer in 5 minutes

We'll notify as soon as your question has been answered.

Plus iconAsk a question to our educators

Badge showing the text 'New'Learn Chemistry with Video Lessons

A-Level Physical Chemistry
1hr 9m · 7 videos
Ibrahim's profile picture
Ibrahim Dangra
·

610 students helped

A-Level Physical Chemistry
GCSE Chemistry: The Basics
12m · 2 videos
Beatrix's profile picture
Beatrix Huissoon
·

868 students helped

GCSE Chemistry: The Basics

Premium video lessons available now on Scoodle

50% discount available

Scoodle's video lessons make learning easy and fun. Try it for yourself, the first lesson is free!