Thermal Physics Ib Dp Lab

The aim of the experiment was to find out how changing the mass effects the rise of the temperature of water.

From the above output, we can see that the p-value is 0.000186, which is smaller than 0.05 (if we select a 0.05 significance level).

This produces a 106% error causing a very large range of possible values causing our results to be very imprecise.

I found out that both of my experiments were off by 0.46 and 0.13 but were remotely

In order to measure the heats of reactions, add the reactants into the calorimeter and measure the difference between the initial and final temperature. The temperature difference helps us calculate the heat released or absorbed by the reaction. The equation for calorimetry is q=mc(ΔT). ΔT is the temperature change, m is the mass, c is the specific heat capacity of the solution, and q is the heat transfer. Given that the experiment is operated under constant pressure in the lab, the temperature change is due to the enthalpy of the reaction, therefore the heat of the reaction can be calculated.

    One possible source of error that can affect the results was that a mercury thermometer was used instead of an electronic one. The use of a mercury

In this lab experiment our main focus was to get skillful in using tools such as the metric ruler, balances, thermometer, and graduated cylinder to capture measurements of length, mass, temperature and volume. Additionally, this lab helped us to become more familiar with the uncertainty of measurements, as well as becoming efficient with rounding our measurements to the correct numbers of significant figures. Our results are measured consistently with rounding to the closest answer we could possibly acquire as the data can tell you.

For q, you found how much heat was gained by the water so you know that same amount of heat was lost by the metal. Therefore, qmetal = -qwater. The mass of the sample was recorded from the baggie. The temperature change

There were three different runs in order to have comparable data and to increase the validity of the experiment. The first run gave 39% of Sodium Bicarbonate. The second run gave 34% of Sodium Bicarbonate while the third one gave 39%, which is the same as the first run. The average percentage was 37% which is much lower than the manufacturer's percentage of 59%. The percent error came out to be -37%.

C. An unknown, rectangular substance measures 3.6 cm high, 4.21 cm long, and 1.17 cm wide.

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

2.68 0.75 69.69 4.83 105.26 50.56 94.69 135.65 6.58 1.24 0.71 0.64 4.84 1.30 41.97% 16.13% 8.32% 12.99% 35.22%

Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to

To achieve this, the final value from each thermocouple was set to be equal to the warm water bath temperature (370C), and the initial reading was set equal to the ice water bath temperature. Thus, for each thermocouple an equation was obtained using the two points to convert voltage readings to temperature. An example of the calibration for one of the thermocouples is shown in Appendix II.

Overall, the experiment succeeded that the metals show the theoretical properties. Differences existed in the mathematical calculation of the actual length. These differences, however, it can be accounted for by experimental error; more over there are uncertainty on purity of the