Measure the time it takes to completely dissolve. Record time in data table. Cold Water: Fill beaker with 80mL if ice water. Use thermometer to record temperature of water. Record the temperature.
Set the stopwatch to 1 minute. Use a lighter to light the fuel. Blow out the fire when the timer reaches 1 minute. Measure the final temperature of the water using a thermometer. Then measure the final mass of the fuel using a mass scale.
At the same time, place the second thermometer bulb just at about the bottom of the beaker 6. Record the initial temperature near the bottom 7. Place ONE drop of food coloring at the bottom of the beaker after the initial 90 second beaker warm-up period *LEAVE THE BEAKER BURNER ON THE HOT PLATE THROUGHOUT THE 3 MINUTES OF TEMPERATURE MEASUREMENTS 8. Record your observations 9.
He placed the his temperature scale at o degree for the boiling point, and ent downward and placed the freezing point at 100 degrees 10. What did the physicist Amonton contribute to the understanding of hot and cold? Amonton was doing heating, and cooling experiments. He saw that when he cooled the object that when the temp dropped so did the pressure. So he thought what would happen if you kept pushing the pressure back.
5. Repeat until the mass is consistent. Data and Observations: Measured melting point | 93.0 ̊ C | Real melting point | 92.5 ̊ C | Mass of evaporating dish | 47.01 g | Mass of evaporating dish and crushed alum | 49.13 g | Mass of crushed alum | 2.12 g | Mass after 1st heating | 48.17 g | Mass after 2nd heating | 48.16 g | Mass of water driven off | .97 g | Mass of anhydrous alum | 1.15 g | Moles of H2O | .0539 moles | Moles of AlK(SO4)2 | .0045 moles | Mole ratio; H2O/AlK(SO4)2 | 12.0 | During the heating of the crushed alum in the hot water bath, the alum had liquefied. The boiling point temperature that was determined was 93.0 degrees Celsius. This process had taken a long time, but around 90 degrees
Reactions Lab David Vaghari INSTRUCTOR: Dr. Chernovitz Monday, July 23, 2012 Oxygen Production Introduction In this lab, potassium chlorate will be decomposed producing oxygen gas and potassium chloride. The hypothesis is that the reaction will yield 3.916 grams of oxygen gas. Materials Test tube 10 grams potassium chlorate Bunsen burner Procedure Step 1. Obtain a test tube, place a 10 gm of potassium chlorate. Step 2.
Try to rinse the precipitate in the funnel until the pink color is gone 12. Place funnel in the drier provided until it is completely dry 13. Let cool to room temperature 14. Weigh the funnel and record the weight 15. Subtract the weight of the funnel and the filter paper from this weight to get the weight of the precipitate Results: wt.
A voltmeter was used to measure the electrical resistance of different solutions. * Experiment and Observation: The plastic and glassware used in this experiment was thoroughly washed with hot water and rinsed with distilled water. * * Part I: Preparation of Standard Phosphate Solutions 1. 1.0 ppm standard: 1.00 mL of 10.0 ppm phosphate solution was placed in a 25 mL graduated cylinder and diluted to exactly the 10 mL mark with distilled water then poured into a plastic cup labeled 1. Cylinder was rinsed with distilled water.
Use 10 mL of the stock and dilute to 1 L with distilled water. This gives a 0.01 M solution. 7. Yeast suspension: Add 1 package of dry yeast to 250 mL of 1% sodium bicarbonate solution. Mix thoroughly and swirl when dispensing.
To begin the ammonium hydroxide test, 15M NH4OH was added to one sample of each cation solution until the formation of a precipitate was observed, with care not to exceed 20 drops. 10 additional drops were added to solutions which formed a precipitate. In order to conduct the cation confirmation tests a Bunsen burner was connected to the desktop gas jet and lit with a striker. A nichrome wire loop was submerged in HCl then placed over the burner flame until no visible color change in the flame was evident. This was repeated after each individual confirmation test to remove any