So we started class by looking over two of the problems from the worksheet: 8 and 9.
Mr. Liebs explained that problem 8 can be done by setting the amount of energy for copper equal to the amount of energy for water. Knowing that, you can use the law of thermodynamics to solve for the mass of water:
q Copper = q Water
(110)(0.2)(57.5)=(4.18)(2.6)(m)
m= ______
In problem 9, you find the specific heat capacity using the law of thermodynamics again. Once you have calculated the specific heat capacity, you convert moles (because the question asks for you to solve for the molar heat capacity of mercury). You can easily convert it by knowing that the unit for specific heat capacity is J/g C and that the grams of mercury is over 1 mole:
585J=(125.6g)(53.5-20.0) c
c= 0.14 J/gC
0.14J/gC x 200.51g/1 mole = ______
Check the answers on moodle!
After the worksheet, we moved onto our lab: The Specific Heat of Metals Lab
We were assigned to work with our partners and follow the procedures from the lab, which was basically just to...
1. collect a dry test tube and measure the mass
2. mass the test tube with a given metal
3. heat up a beaker full of water until it is boiling
4. Put the test tube inside the boiling water for 10 minutes
5. Fill a calorimeter with about 50 mL of water and measure its volume
6. Then measure the initial temperature
7. After the 10 minutes are up, place the test tube inside the calorimeter and measure its final temperature.
After recording each of these measurements, complete the rest of the lab for homework.
The next scribe is... Paige H.
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