When 0.250 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 177 kJ of heat are released. Calculate the value of Delta H for this reaction, as written.

Question

2CH4(g)+3Cl2(g)-->2CHCl3(l)+3H2(g)

delta H=?

Answer 1

If 1/4 mole releases 177 kJ, then 1 mole will release 4x that and 2 moles will release 8x that. Check my thinking.

Answer 2

+1420kJ?

Answer 3

I get 1416 kJ. If you rounded your answer because of significant figures, showing it as 1420 won't do it. Most texts recommend writing it as 1.42 x 10^3 kJ.

Answer 4

hhmm would it be 4x that amount and not 8? im confused

Answer 5

moles = grams/molar mass
0.25 = g/16 and grams = 0.25 x 16 = 4 grams.
The equation as written is 2 moles CH4 so that is 16 x 2 = 32 grams.
177 kJ (for the reaction for the 4 grams) x (32/4) = ??

Answer 6

i guess the teacher put a bad answer bank none of the answer are 1416 but i get what you are saying i will bring this up to him thanx

Answer 7

Try 1.42 x 10^3 kJ and let me know.

Answer 8

I am hoping that this could help you. I had to shorten the link because it was reaching the character limit.

bit.ly/3dD2rEp