# 6.03 chemistry

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6.03 chemistry
Data and Observations
:
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

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