i'm a bit confused in this problem. i think i know how to solve it, but i don't know if what i am doing is correct. please help.
here's the problem:
A 1.50g sample of NH4
is added to 35.0g of h2
in a coffee cup calorimeter and stirred until it dissolves. The
temperature of the solution drops from 22.7°
C to 19.4°
is the heat of solution of NH4
, that is, what is the ΔH for
I tried using the formula qrxn
my value for m is the sum of the grams of ammonium nitrate and water, which is 36.5g.
my value for s is the sum of the specific heats of ammonium nitrate (1.77J/g°C) and water (4.186 J/g°C) which would be 5.956J/g°C.
ΔT would be the difference of 19.4°C and 22.7°C.
therefore, the value for q would be 220.694J.
since ΔH = qrxn
ΔH = 220.694J / (1.50g / 80.04g/mol)
= 11.8 kJ/mol
am i correct? thanks...