When 5.00 g of NaOH(s) are added to 100 g of water using a calorimeter (with Cp = 493.24 J/K), the temperature rises from 25.0 to 37.5 °C. Calculate the molar heat of solution.
Assume that the specific heat capacity of water is 4.18 J/gK and that of the NaOH(aq) solution is the same.
1) qp = Cp∆T,
2) | Heat Lost by Hot Water | = | Heat Gained by Cold Water | + | Heat Gained By Calorimeter |
The Attempt at a Solution
Heat Gained By Solution:
(100 g H2O) x (4.18 J/gK) x (37.5 - 25)K = 5486.25 J
Heat Gained By Calorimeter:
Using qp = Cp∆T,
Cp∆T = (493.24 J/K) x (37.5 - 25)K = 6165.5 J
| Heat Lost | = 5486.25 J + 6165.5 J = 11 651.75 J = 11.65175 kJ
Molar mass of NaOH = (22.99 + 16.00 + 1.01) = 40
5.00 g NaOH x (1 mol ÷ 40g) = 0.125 mol
11.65175 kJ ÷ 0.125 mol = 93.214 kJ/mol
I was just wondering if I did that correctly. I don't actually know the correct answer, but one of my fellow students got a different answer and I'm unsure if I'm the one with the wrong answer or not.
If this isn't the way to find ∆H, could someone show me how or perhaps point me to a useful page on the internet?