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A calorimeter contains 31.0 mL of water at 11.0 degrees C. When 2.00 g of X (a substance with a molar mass of 44.0 g/mol) is added, it dissolves via the reaction

X(s) + H_2O(l)-----> X(aq)

and the temperature of the solution increases to 27.0 degrees C.

Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 J/(g * degrees C}) and 1.00 g/mL] and that no heat is lost to the calorimeter itself, nor to the surroundings.

2007-10-15 05:56:10 · 4 answers · asked by Anonymous in Science & Mathematics Chemistry

4 answers

No. of moles of X = 2.00/44.0 = 0.04545 mol
H = 31(4.18)(27 - 11) = 2073.28 J
Delta H = 2073.28/.04545 = 45.6 kJ/mol

2007-10-15 06:12:54 · answer #1 · answered by DaFreakz 2 · 1 0

delta H = 31 mL 1.0 g/mL x (27-11 degrees) x 4.18

= 31 x 16 x 4.18 Joules

2007-10-15 06:08:47 · answer #2 · answered by ferrous lad 4 · 0 0

Safely & Permanently Remove Moles, Warts and Skin Blemishes

2016-05-17 07:22:12 · answer #3 · answered by Rebecca 4 · 0 0

Use H = mc delta T

2007-10-15 06:08:31 · answer #4 · answered by ag_iitkgp 7 · 0 0

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