Asked by Shirley

2H2(g)+O2(g) ---> 2H2O(l)
delta H= -572kJ/mole of O2

Calculate the amount of heat evolved when 10g of hydrogen are burned in excess oxygen.

Can someone please explain step by step? =D

Answers

Answered by DrBob222
I worked this for you below. You didn't look or you don't understand? If you don't understand, go step by step and be specific about what you don't understand.
Answered by Shirley
I looked at the solution from below but i do not understand where the 4g of H2 came from and why 572kJ x 10/4?

Would you mind explaining please? I'm quite new to this topic.
Answered by DrBob222
Look at the equation.
2H2 + O2 ==> 2H2O
2 mols H2 react with 1 mol O2.
That's 4 g H2 (4*1 = 4) react with 32 g O2 (2*16=32).

So you would get 572 kJ if you had 32 g O2 or 4 g H2. Suppose you had 4 g H2. You would have
572 x 4/4 = ?

Suppose you had twice as much H2 (8 g H2)?
You would obtain twice as much or 572 x 2 = ? How do you get that? It's 572 x (8/4) = ?
If you have 10 g it's 572 x (10/4) = ?

What about apples? If apples cost 5.72 for 4 apples, how much will 10 apples cost? That's $5.72 x (10/4) = ?
Answered by Shirley
Thank you very much, I understand now (:
There are no AI answers yet. The ability to request AI answers is coming soon!

Related Questions