I know I pored this already, but I for it to mention the assumption. See below.
A calorimeter contains 30.0 mL of water at 15.0 C. When 1.50 g of X (a substance with a molar mas of 46.0g/ mol is added, it dissolves via the reaction
X (s) + H2O (l) ----> X (aq)
and the temperature of the solution increases to 26.5 C.
Calculate the enthalpy change for this reaction.
ASSUMPTION:
Assume that the specific heat an density of the resulting solution are equal to those of water and that no heat is lost to the calorimeter itself, not to the surroundings.
Is the delta H negative or positive?
1 answer
I'm not sure I understand the question. The assumptions don't change the way you work the problem; i.e., no heat is lost is obvious and it means density of the solution is 1.00 g/mL which means mass of the solution is 30.0 grams.