CHEM 103 EXPERIMENT 5 GAS LAWS ALL SOLUTIONS WITH EXPLANATIONS + ADDITIONAL NOTES AS PER MARKING SCHEME 2022/2023

CHEM 103 EXPERIMENT 5 GAS LAWS ALL SOLUTIONS WITH EXPLANATIONS + ADDITIONAL NOTES AS PER MARKING SCHEME 2022/2023 NBPL05: Experiment 5 - Gas Laws Purpose: Experiments on different gas laws Notes: ● Robert Boyle Law - pressure of a gas is inversely related to its volume. K is a constant. ● P1V1=P2V2 Demonstration of Bolye’s Law - looking at pressure and volume. ● A syringe is used and it is fitted onto a wooden base and then capped off with a platform. ● Open to the atmosphere - pounds per inch = 14.3 pounds per square inch. ● Volume that is in the syringe with the atmospheric pressure = 33mL is ● Adding to pressure by 2.5 pound weight. Gas gets compressed by the plunger as it gets pushed down. Now it's 27ml with 2.5 pounds on it. ● Total of 5 pounds now the pressure = 22.5 ml ● 7.5 pounds added = 18ml ● 10 pounds added = 16.5ml ● 15 pounds added = 13.0ml ● The higher the pressure added the lower the volume gets. Jacques Charles Law ● V=K*T ● Volume and how the temperature is related. ● As we increase the volume the temperature is going to increase ( balloon example) ● V1/T1 = V2/T2 Demonstration of Charles Law ● Cooling a flask in ice water. ● Tighten clamp stand, added a stopper with thermometer and a syringe inside. ● initial temperature: 6.5 degrees , this is about 328ml in volume ( flask) ● He is going to use a blow dryer to heat the flask and record at every 5 degrees a volume reading - Plunger should raise. ● When it was 6.5 degrees, the plunger was all the way down. ● 36.5 degrees it raised to 23.5ml - we had a 23.5ml increase. This happened because, we cooled the flask to about 6 degrees and the gas expanded with the heat and it pushed the syringe up because it had nowhere else to go. Ideal gas law ● Bringing together Boyle's law and Charles law. ● Ideal gas law : PV=nRT This describes any gas regardless of their identity. ● STP ( standard, temperature, pressure) S temp is 0.0C = 273.15K @ 1 atm ● Rearrange the gas law to V=nRT/P ● V = 1.0mole*0.K/1.0atm = 22.4L mole volume for all gasses. ● N = number of moles which is = to mass of a particular gas / its molar mass. ● n=m/Mm ● PV=nRT ● PV= (m/Mm) X RT ● Mm= mRT/PV Procedure & Results Experiment 1 - calculating the molar mass for acetone ● Flask with foil covering which has a paperclip size hole in the