When 0.678 g of Ca metal is added to 200.0 mL of 0.500 M HCl(aq), a temperature increase of 11.0C is observed.

Question

Assume the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/gC.
(Note: Pay attention to significant figures. Do not round until the final answer.)
The molar heat of reaction, H rxn, for the reaction of

Ca(s) + 2H+(aq) -> Ca2+(aq) + H2(g)

THANKS! :)

Answer 1

q = mass water x specific heat water x delta T.
Then q/0.678 = ?J/g. Convert that to kJ/mole.

Answer 2

OK. I just read your earlier post.
200 x 4.184 x 11 is correct.
And that number divided by 0.678 is correct for J/g.
Just take that number (J/g) and divide by 1000 to convert to kJ, then multiply by molar mass Ca to convert to kJ/mole.

Answer 3

It is negative fyi

Answer 4

why do you multiply by 200? how to the units of mL just disappear then? what do you do with 1.00 g/mL?

Answer 5

just type it in. it works when its negative.

Answer 6

You would times it by the momentum currency of memorandum which is stated in Hess's law of physics