Experiment V

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Portage Learning *

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103

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Chemistry

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Feb 20, 2024

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Chemistry Lab Report Name: Date: 06/06/2022 Experiment #: 5 Title: Gas Law Purpose: To learn and determine the gas laws in this experiment. Procedure: Boyle’s Law P= K/V P 1 V 1 =P 2 V 2 - Plunger’s atmospheric pressure= 33mL o Add 2.5lb weights the volume= 27 mL o Add another 2.5 weights (total of 5lb) = 22.5mL o Add another 2.5 weights (total of 7.5lb) =18mL o Add another 2.5 weights (total of 10lb) = 16.5 mL o Add a 5.0lb weight (total ofb15lb) = 13.0mL Charles' Law - Fill cooling flask with acetone - Initial temperature= 6.5°C - Using a blow dryer apply heat to flask and record the temperature and volume Ideal Gas Law - We need to determine the molar mass of acetone - Weight of flask with foil covering on balance= 112.1373g - Add 1.8 mL of acetone into the flask - Clamp on flask onto a ring stand and put it in a water bath - Acetone has a boiling point of 57°C - Let the flask stay in the water bath until it read 66°C to make sure acetone is vaporized o took 13 minutes o Entire flask was not in water bath so this may cause an error o Final temperature= 66.4°C - Place flask in a cold-water bath to help recondense and vapor acetone - Dry the flask and weigh it o 112.7900g acetone - Now find the molar mass of acetone with the given data

Chemistry Lab Report Measuring Moles of Mass produced by: CaCO 3 (s) + 2 HCl (aq)  CaCl 2 (ag) + H 2 0 (l) + CO 2 (g) - Use a gas apparatus to determine the volume of gas o Has three parts:  Reaction chamber (syringe connected to a test tube)  Gas Buret which allows us to measure gas produced  A leveling bulb which makes sure the levels are equal and is under atmospheric pressure  Make sure there is no leaks Data/Results/Calculations: Boyle’s Law P=K/V P 1 V 1 =P 2 V 2 Pressure in this lab= 14.3 psi Area of syringe head = 0.75in 2 Charles’ Law V= k x T (k=constant) V 1 /T 1 =V 2 /T 2 Initial temperature= 6.5°C Final temperature= 36.5°C Final volume= 23.5mL Ideal Gas Law PV= nRT Molar mass of acetone: M m = mRT/PV m=0.6527g R= 0.08206 L-atm/mol-K T= 66.4°C  339.6 K P= 0.9766 atm V (of flask) = 328 mL  0.328L M m = (0.6527g) (0.08206 L-atm/mol-K) (339.6 K) / (0.9766 atm) (0.328L) = 56.8 g/mol % error= (58.08 g/mol - 56.8 g/mol) / (58.08 g/mol) x 100 = 2.2%

Chemistry Lab Report Molar Mass of CO 2 (g) n= PV/RT P= 0.9766atm V = 48.8 mL  0.0488 L R= 0.08206 L-atm/mol-K T= 295.7K n= (0.9766atm) (0.0488L) / ( 0.08206 L-atm/mol-K ) (295.7K) = 0.00196 mol CO 2 (g) Conclusions: In this lab we were introduce to the three gas laws: Boyle’s law, Charles’ Law, and the Ideal gas law. We use these laws to calculate and find the unknown variables in our experiments. We use the Boyle’s Law to find PSI as known as the atmosphere pressure, which in the experiment we used a syringe and weights. In Charles’ Law we calculate the volume when temperature increases by collecting data from a heated syringe. We also use the Ideal Gas Law to calculate the molar mass of acetone when heated and cool and to find the moles of CO 2 (g) that was produced in a reaction. Notes:  Mercury is used to determine the atmosphere pressure (use to predict the weather)  The higher the pressure the smaller the volume  Pressure units= lb/in 2 aka PSI  Charles’ law: as volume increase, temperature increase.

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