Register
In the following reaction, how much heat is generated when 1.83 moles of CH4 are burned? CH4 (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) Hº = -802 kJ/mol | KJ
101k views
22 votes
In the following reaction, how much heat is

generated when 1.83 moles of CH4 are
burned?
CH4 (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) Hº
= -802 kJ/mol
| KJ

In the following reaction, how much heat is generated when 1.83 moles of CH4 are burned-example-1
User Replay
by
6.6k points

1 Answer

5 votes

Answer:

1470 kJ (to 3 sf)

Step-by-step explanation:

(802)(1.83) = 1470 kJ (to 3 sf)

User Becca Petrin
by
8.1k points
Ask a Question
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.

7.6m questions

10.1m answers

Other Questions

How do you balance __H2SO4 + __B(OH)3 --> __B2(SO4)3 + __H2O
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.
Why is gold preferred as a superior metal over silver and bronze?
What is the evidence of a chemical reaction when the fireworks go off
Link Copied!