Last modified: Wed 12/31/1969 06:00:00 pm ACA

It is OK to use your textbook, but if you can answers the questions without it that is OK too.

Do not press the RETURN or ENTER key while you are answering these questions. Your browser will interpret either the same as clicking on the Submit key.

Answer all of the questions below. If you do not know an answer enter CNA. However, it will help me the most if you answer each question with your best intuition/idea about what would be a reasonable answer.


First Name:

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In this experiment we will collect data that will allow the determination of the specific heat of copper metal. Look at the questions below and then watch the video. When you have the information required to complete a question, pause the video by pressing the spacebar, and record the data. Pressing the spacebar again will re-start the video.

1. Enter the mass of the copper cylinder as measured using the analytical balance. (The mass is around 57 g.)

grams

2. Enter the initial the temperature of the copper (Note the copper is in boiling water...hint, hint.);

°C

3. Enter the mass of the water in the coffee-cup calorimeter as measured using the analytical balance. (The mass is around 188 g.)

grams

4. Enter the initial temperature of the water in the coffee-cup calorimeter;

°C

5. Enter the final temperature of the water in the coffee-cup calorimeter;

°C

6. Enter the final temperature of the copper in the coffee-cup calorimeter;

°C

7a. Which sample, the piece of copper or the sample of water, started at the higher temperature?

b) Which sample, the piece of copper or the sample of water, started at the lower temperature?

c) Which substance, the piece of copper or the sample of water, lost heat?

d) Which substance, the piece of copper or the sample of water, gained heat?

e) Given the relationship that we invented in class, q(heat) = mass*c*T and that 'c' for water, the specific heat, is 4.184 joules/g-1 °C-1, calculate the heat absorbed by the water. (Note: find the experimental mass of water and the temperature change the water experienced from the data above.)

joules

f) How much heat was given off by the piece of copper?

joules

g) Given the relationship that we invented in class, q(heat) = mass*c*T, calculate the specific heat for the sample of copper used in this experiment.

joules/g-1 °C-1

8. Using your textbook or an online resource determine the literature value of the specific heat of copper in joules g-1 °C-1.

joules g-1 °C-1

9. Speculate why the specific heat for copper that you determined from the experiment does not agree with the literature value of the specific heat.

Below is a list of four substances and their specific heats.

 

 Substance Specific heat (joules g-1 °C-1)

Aluminum

Al(s)

0.90

Nitrogen

N2(g)

1.04

Water

H2O(l)

4.184

Methane

CH4(g)

2.20

10. Which substance has the highest specific heat?

11. Assuming equal amounts of all four substances all at the same initial temperature. If the same amount of heat is added to each substance, which substance will experience the largest temperature change?

12. If a sample of water, experiences a change in temperature of 10.0 °C, what will be the temperature change experienced by a sample of solid aluminum that has the same mass?

°C

 

13. Is there anything about the questions that you feel you do not understand? List your concerns/questions.

14. If there is one question you would like to have answered in lecture, what would that question be?