User:Batman-is-my-mom

From Wikipedia, the free encyclopedia

Joseph Stevenson May 27, 2008

The Specific Heat of a Metal Lab

Data and Observations:

Measurements of Mass and Temperature: Trial 1 Trial2 (given) Mass of lead shot 91.80 g 106.08 g Initial temperature of water in cup 23.1 oC 23.2 oC Initial temperature of lead shot (temperature of boiling water) 98.9 oC 99.24 oC Maximum temperature of lead + water 26.1 oC 95.47 oC Mass of water 100.01 g 100 g

Analysis and Conclusions:

1. Determine the changes in temperature of the water (Twater) and of the lead shot (Tlead) for each trial.

Trial 1:

    mlead x Clead x Tlead = mwater x Cwater x Twater

91.8 g x 0.1276 J x (98.9 - Tfinal) oC = 100.1 g x 4.18 J x (Tfinal – 23.1) oC

   g x  oC                               g x  oC

11.71368 (98.9 - Tfinal) = 418.418 (Tfinal – 23.1)

1158.482952 - 11.71368Tfinal = 418.418Tfinal – 9665.4558

430.13168Tfinal = 10823.93875

Tfinal = 25.16424447

Trial 2:

mlead x Clead x Tlead = mwater x Cwater x Twater

106.08 g x 0.1276 J x (99.24 - Tfinal) oC = 100 g x 4.18 J x (Tfinal – 23.2) oC

      g x  oC                                      g x  oC

13.535808 (99.24 - Tfinal) = 418 (Tfinal – 23.2)

1343.293586– 13.535808Tfinal = 418 Tfinal – 9697.6

431.535808Tfinal = 11040.89359

Tfinal = 25.58511573

2. Calculate the heat gained by the water in each trial.

Trial 1:

    mwater x Cwater x Twater = Heat gained by water

100.1 g x 4.18 J x (25.16424447 – 23.1) oC = Heat gained by water

             g x  oC

418.418 (2.06424447) J = Heat gained by water

        863.7170426 J = Heat gained by water

Trial 2:

mwater x Cwater x Twater = Heat gained by water

100 g x 4.18  J x (25.58511573  – 23.2) oC  = Heat gained by water
        g x  oC

418 (2.38511573) J = Heat gained by water

        996.9783751 J = Heat gained by water

3. Remembering that the heat gained by the water equals the heat lost by the lead, calculate the specific heat of lead for each trial.

Trial 1:

      Heat lost = Clead

Mlead x Tlead

863.7170426J = Clead 91.80 g x (98.9 - 25.16424447) oC

863.7170426 J = Clead 91.80 g x (73.7358) oC

863.7170426 J = Clead 6768.9846 g x oC

0.1276 J = Clead g x oC

Trial 2:

       Heat lost = Clead

Mlead x Tlead

996.9783751 J = Clead 106.08 g x (99.24 - 25.58511573) oC

996.9783751 J = Clead 106.08 g x 73.6549oC

996.9783751 J = Clead 7813.3118 g x oC

0.1276 J = Clead g x oC