A community for students.
Here's the question you clicked on:
 0 viewing
Yahoo!
 3 years ago
Complete combustion of 5.90 g of a hydrocarbon produced 18.8 g of CO2 and 6.75 g of H2O. What is the empirical formula for the hydrocarbon?
Yahoo!
 3 years ago
Complete combustion of 5.90 g of a hydrocarbon produced 18.8 g of CO2 and 6.75 g of H2O. What is the empirical formula for the hydrocarbon?

This Question is Closed

Yahoo!
 3 years ago
Best ResponseYou've already chosen the best response.0Lol...@Rohangrr Wat Do u Mean..)

Yahoo!
 3 years ago
Best ResponseYou've already chosen the best response.0Any Idea @VincentLyon.Fr

VincentLyon.Fr
 3 years ago
Best ResponseYou've already chosen the best response.2It is very easy, and you do not even need the information about the 5.9 g of hydrocarbon. It is just a matter of proportionality. Look how you solve this kind of problem. 1. Write general chemical equation: \(\large C_nH_m+xO_2\rightarrow nCO_2+\frac m2 H_2O\) 2. Work out proportionality of masses using molar masses 44 g/mol for carbon dioxide and 18 g/mol for water: Mass of \(CO_2\) produced is 44n Mass of \(H_2O\) produced is 18m/2 = 9m Hence: \(\Large \frac{44n}{9m} = \frac{18.8}{6.75}\) => \(\Large \frac mn = \frac 74\) 3. After rearranging for a simple fraction 7/4 : Empirical formula is \(C_4H_7\)

VincentLyon.Fr
 3 years ago
Best ResponseYou've already chosen the best response.2Note: if mass of oxygen used is mentioned, you might have to write the stoichiometric coefficient for oxygen as n + m/4 I was just lazy because is was not useful in your example !
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.