Stuck On Thermochemistry Question?

Posted on 2015-12-01 07:16:00 in Chemistry by STEVEN FORD

Part A:
A calorimeter contains 24.0 mL of water at 15.0 ?C . When 1.90 g of X (a substance with a molar mass of 78.0 g/mol ) is added, it dissolves via the reaction

X(s)+H2O(l)?X(aq)
and the temperature of the solution increases to 25.0 ?C .

Calculate the enthalpy change, ?H, for this reaction per mole of X.

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

Part B:
Consider the reaction

C12H22O11(s)+12O2(g)?12CO2(g)+11H2O(l)
in which 10.0 g of sucrose, C12H22O11, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/?C. The temperature increase inside the calorimeter was found to be 22.0 ?C. Calculate the change in internal energy, ?E, for this reaction per mole of sucrose.

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