Log in
Chemistry
1
answer
0
watching
709
views

When hydrocarbons are burned in a limited amount of air, both CO and CO2 form. When 0.450 g of a particular hydrocarbon was burned in air, 0.467 g of CO, 0.733 g of CO2, and 0.450 g of H2O were formed. (a) What is the empirical formula of the compound? (b) How many grams of O2 were used in the reaction? (c) How many grams would have been required for complete combustion?

Watch
1
answer
0
watching
709
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Avatar image
Liked by ronyjamwal2002
Nestor Rutherford
Nestor RutherfordLv2
27 May 2020

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

1) When 6.580 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 20.16 grams of CO2 and 9.631 grams of H2O were produced.

In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

2)When 2.823 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 8.859 grams of CO2 and 3.627 grams of H2O were produced.

In a separate experiment, the molar mass of the compound was found to be 70.13 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

When 4.524 grams of a hydrocarbon,CxHy, were burned in a combustion analysisapparatus, 14.19 grams of CO2 and5.811 grams of H2O were produced.

In a separate experiment, the molar mass of the compound was foundto be 56.11 g/mol. Determine the empirical formulaand the molecular formula of the hydrocarbon.

When 6.224 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.04 grams of CO2 and 4.308 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 78.11 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in