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Will the recorded temperature change for an exothermic reaction performed in a glass calorimeter be greater or less that?
The recorded temperature change for an exothermic reaction performed in a glass calorimeter is less than the Styrofoam cup calorimeter. This is because the glass will conduct heat away more than the Styrofoam.
How can I make a styrofoam calorimeter?
To make a styrofoam calorimeter, you will need a styrofoam cup, a lid for the cup, a thermometer, and a stirrer. Cut a hole in the lid to insert the thermometer. Fill the cup with a known volume of water and record its initial temperature. Place the cup in a larger container filled with water and heat or cool the water to a desired temperature. Place the lid on the cup and stir the water to ensure even temperature distribution. Record the final temperature of the water to calculate the heat exchange.
How can I make a calorimeter?
To make a calorimeter, you will need a container to hold water, a thermometer to measure temperature changes, and insulation to prevent heat loss. You can use materials like a Styrofoam cup, a thermometer, and a lid to create a simple calorimeter for measuring heat energy.
What kind of cup would you use to make a calorimeter?
Styrofoam Cup
What kind of cups would you use to make calorimeter?
Styrofoam Cup
How can styrofoam be dissolved using acetone?
Styrofoam can be dissolved using acetone because acetone breaks down the chemical structure of the styrofoam, causing it to dissolve.
How can you create a homemade calorimeter for measuring heat transfer in chemical reactions?
To create a homemade calorimeter for measuring heat transfer in chemical reactions, you can use a Styrofoam cup as the container. Place a thermometer inside the cup to measure temperature changes during the reaction. Insulate the cup with a lid to prevent heat loss. Record the initial and final temperatures to calculate the heat transfer.
How would a calorimeter constant be effected if it were made of glass instead of styrofoam?
If a calorimeter were made of glass instead of styrofoam, its calorimeter constant would likely be higher. This is because glass has a higher thermal conductivity compared to styrofoam, allowing for faster heat transfer between the system and its surroundings. As a result, the glass calorimeter would require a higher constant to account for this increased heat loss or gain.
Why did you need to transfer the metal quickly from the hot water bath to water in the styrofoam cup calorimeter?
You need to stir the water because the heat energy coming off whatever you put into the calorimeter (whether it be food, metal, etc.) won't evenly distribute its heat throughout the water, and therefore the temperature reading won't be as accurate. If you stir it, the heat will be more evenly "mixed in" with the water, so to speak, and you will get a more accurate reading.
In two or more complete sentences explain to someone who knows nothing about heat transfer how to construct and use a constant pressure calorimeter.?
It is a very simple device; basically it can be made from two styrofoam cups, a stirrer and a thermometer. Placing the two styrofoam cups inside each other (for insulation), a chemical reaction in a liquid medium (typically water) is performed in the inner cup, and the change in temperature recorded.
Why are styrofoam cups good for testing calorimetry of bombs?
Because syrofoam is a good insulator so it keeps most of the heat in the calorimeter. It also has a low specific heat
What is the best way to measure calorimetry?
Calorimetry is the scientific practice of measuring the heat that a reaction between energies may create, and there are two different types of measurements one can take; they are based on constant pressure and constant volume. To measure calorimetry, one should employ the use of a calorimeter (which is basically an insulated object like a styrofoam cup). One must then seal the reactants in the calorimeter and measure the change change in temperature, comparing the previous temperature to the temperature after the experiment.
