6.03 Calorimetry Lab

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The result of adding iron filings to an aqueous solution of copper sulfate(II) sulfate and adding iron sulfate and copper will be used in a single replacement action. Also it should be able to find the ratio of moles of a reactant to moles of a product in the chemical reaction. Thus, it should answer another purpose for the lab which is to find is to be able to relate this ratio to the coefficients of these substances in the balanced equation for the reaction.
Hypothesis: Both of coefficient off iron
Variables:
Procedure

Find the mass of a clean, dry 100 ml beaker. Record the mass on the data table.
Measure out approximately 8 grams of copper sulfate crystals (CuSO4) and add these to the beaker, measured before.
Measure 50 ml of water in a graduated cylinder and add it to the crystals in the beaker. …show more content…
Heat the mixture in the beaker to just below boiling. Do not allow the liquid to boil.
Continue heating and stir the mixture until the crystals are completely dissolved.
Using the balance, tare a weighing dish and measure out approximately 3 grams of iron dust. Record your exact mass in the data table.
Add the iron dust, small amounts at a time, to the hot copper sulfate solution. Stir continuously. After all the iron has been added and the mixture stirred, allow the beaker to sit for 10 minutes while the reaction proceeds. Record the observations in the data table.
Decant the liquid into a 250 mL beaker. Do not allow any solid to pass over to the 250 ml beaker.
Add about 10 ml of water to the solid in the 100 mL beaker. Stir vigorously in order to wash off the solid. Let the solid settle and again decant the liquid.
Spread the solid out on the bottom of the beaker, label the beaker, and place the beaker on the tray to dry.
After the mixture is dried, find the mass of the beaker and the dry copper metal. Record in the data

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