Consider the combustion of propane:

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O(l) ΔH = –2221 kJ

Assume that all of the heat comes from the combustion of propane. Calculate ΔH in which 5.00 g of propane is burned in excess oxygen at constant pressure.

0 0
Add a comment Improve this question Transcribed image text
Answer #1

The reaction of combustion of propane is

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O(l)        ΔH = –2221 kJ

The enthalpy of combustion of 1 mole of propane is -2221 kJ.

Number of moles of propane in 5 g of propane = 5/44.1 = 0.113 mol

Therefore, dH for 5 g (0.113 mol) of propane = –2221 x 0.113 kJ = - 251.81 kJ

Add a comment
Know the answer?
Add Answer to:
Consider the combustion of propane: C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O(l) ΔH...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
Active Questions