# 6.03 chemistry

:

Part I:

Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part I. Metal

Aluminum

Zinc

Iron

Cooper

Mass of metal

27.776 g

41.664 g

34.720 g

41.664 g

Volume of water in calorimeter

26.0 mL

26.0 mL

26.0 mL

26.0 mL

Initial temp. of water in calorimeter

25.3 degrees C

25.3 degrees C

25.3 degrees C

25.3 degree’s C

Temp of hot water and the metal

100.5 degrees C

100.5 degrees C

100.5 degrees C

100.5 degrees C

Final temp in the calorimeter

31.6 degrees C

34.8 degrees C

33.1 degrees C

34.5 degrees C

Part II:

Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part II. Metal

Metal A

Metal B

Metal C

Mass of metal

15.263 g

26.605 g

20.484 g

Volume of water in calorimeter

24.0 mL

24.0 mL

24.0 mL

Initial temp of water in calorimeter

25.2 degrees C

25.3 degrees C

25.2 degrees C

Temp of hot water and metal

100.3 degrees C

100.3 degrees C

100.3 degrees C

Final temp in the calorimeter

27.5 degrees C

32.2 degrees C

28.0 degrees C

Calculations:

Show your work and write a short explanation with each calculation. Part I:

1. Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. The water has absorbed the heat of the metal. So, qwater = qmetal m=mass of water= density x volume = 1 x 26 = 26 grams

ΔT = T(mix) – T(water) = 38.9 – 25.3 = 13.6

q(water) =26 x 13.6 x 4.18

q(water) = 1478 Joules

2. Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation. qmetal = - 205 J = 15.363 g x C x (27.2 – 100.3 C)...

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