Q = m. c. T Q cu solution = (3.96 J /( g C ))×150 g ×(53.2 C 26.6 C ) = 7095.43

ID: 924732 • Letter: Q

Question

Q = m.c.T

Q cu solution = (3.96 J/(g C))×150 g ×(53.2C26.6C) = 7095.43 J

Q Al = (3.96 J/(g C))×0.822 g ×(53.2C26.6C) = 86.58 J

Qcalorimeter = (QCu solution+QAl) = (7095.43 J+86.58 J) = 7008 J

Qreaction = Qcalorimeter

delta H = -7008J

Q = m.c.T

Q cu solution = (3.96 J/(g C))×150 g ×(56.1C26.7C) = 17463.6 J

Q Al = (3.96 J/(g C))×0.844 g ×(56.1C26.7C) = 98.26 J

Qcalorimeter = (QCu solution+QAl) = (17463.6 J+98.26 J) = 17365.34 J

Qreaction = Qcalorimeter

delta H = 17365.34 J

Is this an exothermic or an endothermic reaction? Does the sign oof you delta H shown in your calculations correctly indicate this? Why?

Since Hrxn are negatvie for both cases... both substances are exothermic, meaning they will release heat.

YES, it correctly shows that heat is being released to the surroudings

Qsurr = -Hrxn

the heat being lost by system = heat being gain by surroundings

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