Register

What is the molecular formula of a compound containing 42.17% Chlorine, 57.83% Oxygen, and has a molecular mass of 166 g/mol?

What is the molecular formula of a compound containing 42.17% Chlorine, 57.83% Oxygen, and has a molecular mass of 166 g/mol?
39.5k views
3 votes
What is the molecular formula of a compound containing 42.17% Chlorine, 57.83% Oxygen, and has a molecular mass of 166 g/mol?

User Tim Barnett
by
7.8k points

1 Answer

5 votes

Answer:

C2H4CL2

Step-by-step explanation:

this is your answer

User Arcord
by
8.8k points
← Prev Question Next Question →

Related questions

Ask a Question
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.

9.4m questions

12.2m answers

Categories

Other Questions

Compare and contrast an electric generator and a battery??
Can someone complete the chemical reactions, or write which one do not occur, and provide tehir types? *c2h4+h2o *c3h8 + hcl *c2h2+br2 *c4h10+br2 *c3h6+br2
As an object’s temperature increases, the ____________________ at which it radiates energy increases.
Link Copied!