Stephanie+and+JC

= ​ Calorimetry=


 * Participants**: Stephanie and JC
 * Purpose**: The purpose of this lab is to inquire about calorimetry.


 * Brief Description of Experiment**: Basically we took the calorimeter that was given and added room temperature water to it. Then we took the temperature of the water and recorded. After that we took a piece of heated metal and added it to the system, making sure to quickly close the lid to optimize the experiment. We then took the end temperature of the system and repeated.

__-Trial 1-__ -__Trial 2-__ -__Trial 3-__ 245.82 **234.23 *260.3- -Initial With Water (g)- Temperature (c) - 24.7 24.3 24.3
 * Data**:
 * 62.69* *62.23- *62.34- -Mass of Inner Chamber (g)-
 * 27.9*** *28.4* **28.0- -Final Temperature (c) -
 * 112.71 112.15* 114.76- Mass Of Metal (g)-
 * 100*** *100* 100* -Temperature of Metal (c)-

NOTE- this table is really hard to read, but this was the best i could do. The little are for place holders because the thing won't save with spaces.

**Results**:

After adding the room temperature water to the calorimeter and then adding the piece of 100 degree celsius metal, we were able to watch the water and metal experience a change in temperature. The water gained heat from the hot metal and the metal lost heat to the water. In the three trials that were done with these, a pattern began to form. We noticed that each time, the room temperature water, approx. 24.5°C, always evened out at right about 28°C with the added heat from the metal.


 * Lab Questions**:

1. In what ways did you attempt to make your result as accurate as possible? Describe how each way contributed to a more accurate result.

One way was to close the cover of the calorimeter as soon as possible after the metal was dropped in, so as to ensure minimal heat escaped.

2. In what ways does the calorimeter fail as a closed system? What mathematical effect on your result would these failures have?

The calorimeter failed as a closed system because it wasn't completely sealed and there were holes in the top for the thermometer and mixer. These aspects could have an effect on the readings given and ive us innacurate data temperature-wise.

3. Suppose you were asked to measure the latent heat of vaporization of water (the amount of heat required to turn liquid water into a gas). You propose to do this by heating a bar of the metal used in this experiment to a very high temperature (500oC) and dropping it into a calorimeter with water initially at 95oC. Describe what you think will happen and what measurements you would need to make in order to calculate the latent heat. Approximate how much water would be turned to steam if the bar had a mass of 0.7kg and the final temperature of the 0.35kg of water in the calorimeter was 100oC.

The boiling pont of water is 99.97 degrees celsius, and if the water is already at 95 degees celsius on its own, it is not going to take much to get it to that temperature. You would have to know the mass of the 500 degree bar, and you would also need to calculate the mass of water trying to be heated.

** Conclusion **:

Our results could be easily reproduced if you used the same piece of metal at the same temperature, and if the calorimeter was the same with all the same temperatures of water. This would reproduce similar, or exact, results because there is no change in the experiment. Our results would differ from and accepted becasue of human error, such as temperatures or readings. To improve results and make them closer to the acceoted would be to minimize the time that the metal is out of the water, or to minimize the time that the top is off of the calorimeter.

//Don't forget to link to your lab report from the lab reports page and to include a link to your lab report in your reflection.//