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
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4 answers
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asked by
Anonymous
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Science & Mathematics
➔ Chemistry