Heat the beaker on a hot plate set to medium. (Setting 4). Stir with a glass-stirring rod while heating. When a solid appears, stop heating. 8.
Write a hypothesis on what you think will happen when mixed. 3. Place the magnesium ribbon ni the hydrochloric acid; record observations. Sugar and Heat 1. Add a bit of sugar to aluminum foil and fold the edges so it is covered from the sides.
10-29-10 Analysis of Alum Purpose: To determine if the sample crystals are really aluminum potassium sulfate or alum. Materials: alum, beaker, hot plate, thermometer, thermometer clamp, mortar, pestle, capillary tubes, small rubber bands, stirring rob, goggles. Procedure: Determine the melting point: 1. Pulverize with pestle about 2.00 grams of alum. 2.
3. Set up the ring stand, iron ring, and clay triangle to support a crucible over the Bunsen burner. 4. Place the clean and empty crucible with its cover on the clay triangle. Turn the Bunsen burner on and ignite it.
10/8/13 Lab Report Introduction The purpose of the experiment was to do three different reaction and calculate the enthalpy change of the reaction with Hess’s Law. Then compare your calculated results to the results from the experiment. Experimental Design Materials: Vernier computer interface Computer Temperature Probe Two styrofoam cup 100 mL graduated cylinders Glass stirring rod 2.0 M Hydrochloric acid, HCl, solution 2.0 M Sodium Hydroxide, NaOH, solution 2.0 M Ammonium Chloride, NH4Cl, solution 2.0 M Ammonia, NH3, solution Ring Stand Utility Clamp Fume hood or well-ventilated room Magnetic Stirrer Paper Lid Procedures: Use proper lab safety and wear safety glasses, and make sure in well-ventilated room. Connect the temperature probe to the Vernier interface in the Channel 1 port. Then connect interface to the computer using the USB cable.
Roll the magnesium into a loop and thread the string through the Magnesium and tie it off. Be sure to leave several centimeters of thread free to use as a “handle”. 5 Assemble a ring stand and clamp for supporting the gas collection tube. 6 Completely fill a large beaker to the
Lab 2: If we heat sand then conduction will occur. III. Materials Lab 1: * 500mL Beaker * Water * Hot Plate * 2 Thermometers * Food coloring * Stopwatch * Oven mitt Lab 2: * 500 Ml beaker * Water * Hot Plate * 2 Thermometers * Beaker of sand – about 150-200 mL * Stopwatch * Oven mitt IV. Procedure Lab 1 1. Gather all materials 2.
We utilized crucibles, crucible lids, clay triangle and the technique of bending down the edges of the triangle. This setup allowed us to expose Epsom salt to high heat in a vessel designed for high temperature exposure. Reagents. We used a small carton of Epsom salt provided by the stockroom and a large blue bag of Epsom salt provided by the instructor. Safety Considerations.
Then weigh the crucible without the hydrate after heating. Record both masses. Next, add CoCl2 ∙6H2O and weigh the crucible. Now place the hydrate and crucible on the hot plate. Observe the color change while it is being heated.
Introduction In this lab I observed the burning of a candle very closely. I found out that the candle needs oxygen to burn, that it produces carbon dioxide similar to the way that my body produces carbon dioxide, and that a candle produces water as a second waste product. I learned that if I hold an object in the flame it becomes covered with soot which is unburned carbon fuel. Finally, I learned that neither the solid wax, nor the melted wax, nor the wick burns when a candle is lit. In fact, the wax itself is burning as a vapor or gas.