Purpose
The purpose of this experiment is to confirm the functional relationship of Boyle’s law through the use of a manometer. The two parts of this experiment will determine the number of moles of oxygen and the second part will determine the number of moles of nitrogen, that will lead to determine the value of R by measuring P, V, and T.
Theory/Principles
A physical law such as Boyle’s law states that P, the exerted fixed mass of gas at a constant temperature and V, the volume have a relationship. Their kind of relationship is V=f(P) relationship and it is believed that PV go together to remain constant. A water manometer is an instrument used to measure pressure. The model of kinetic theory of gases helps elaborate one of the most difficult …show more content…
Add the tap water into the bulb and gas buret so it contains the water. Take a clean hard glass tube with one end sealed and the other fine polished and load it into it between a 0.10g and 0.15g of potassium chlorate. Place the chlorate down the tube with spatula and tap it until it is down to the bottom. Weigh the tube. Attach the tube with chlorate to the leveling bulb and level the bulb 10cm below and match up the water levels in the bulb and buret and the read the gas level.
Data
Part A:
Uncalibrated Volume, V u 4.1mL
Volume of air in buret when levels are equal, V_o 40.5mL
Volume of air in bure at different pressures, V +1 36.50mL
Volume of air in bure at different pressures, V −1 45.7mL
Height difference between water levels,h +1 41 cm
Height difference between water levels,h −1 109 cm
Temperature of water, T 25.0°C
Barometric Pressure, P atm 710.0 mmHg
Part B:
Mass of tube + KClO3
6.1029 g
Mass of tube + residue after heating 6.1920 g
Initial gas level in buret (mL) 44.5 mL
Final gas level in buret (mL) 49.7 mL
Room Temperature ( C °) 22.6°C
Barometric Pressure mm Hg) ( 710.0 …show more content…
We were able to determine the moles of a gas which resulted to 5.5x〖10〗^(-3)mol O_2. This led to a R constant, 2.1 x 〖10〗^(-2) (atm∙L)/(mol∙K). Graph 1 did not result as linear as expected but it did have a negative slope to an extant which demonstrated that as the volume gets higher then the pressure decreases. Graph 2 and 3 did have a more positive slope proving that as the pressure increases, the 1/V and PV also increased. The graphs do not appear to be straight lines as Boyle’s law states meaning our results had errors that did not strengthen or support the law but it did demonstrate that they can have a relationship just proper instructions need to be followed.
Conclusion
In conclusion, determining constant was not as easy as assumed with just one wrong number it can change the direction of graphs and misinterpret if PV have a relationship. This experiment did have unavoidable errors such as both gross and systematic errors. The equipment used in this experiment was not as accurate as the ones needed and also the technique used could not be as précised. One may try to avoid errors by continuing with more determinations.
The purpose of this experiment is to confirm the functional relationship of Boyle’s law through the use of a manometer. The two parts of this experiment will determine the number of moles of oxygen and the second part will determine the number of moles of nitrogen, that will lead to determine the value of R by measuring P, V, and T.
Theory/Principles
A physical law such as Boyle’s law states that P, the exerted fixed mass of gas at a constant temperature and V, the volume have a relationship. Their kind of relationship is V=f(P) relationship and it is believed that PV go together to remain constant. A water manometer is an instrument used to measure pressure. The model of kinetic theory of gases helps elaborate one of the most difficult …show more content…
Add the tap water into the bulb and gas buret so it contains the water. Take a clean hard glass tube with one end sealed and the other fine polished and load it into it between a 0.10g and 0.15g of potassium chlorate. Place the chlorate down the tube with spatula and tap it until it is down to the bottom. Weigh the tube. Attach the tube with chlorate to the leveling bulb and level the bulb 10cm below and match up the water levels in the bulb and buret and the read the gas level.
Data
Part A:
Uncalibrated Volume, V u 4.1mL
Volume of air in buret when levels are equal, V_o 40.5mL
Volume of air in bure at different pressures, V +1 36.50mL
Volume of air in bure at different pressures, V −1 45.7mL
Height difference between water levels,h +1 41 cm
Height difference between water levels,h −1 109 cm
Temperature of water, T 25.0°C
Barometric Pressure, P atm 710.0 mmHg
Part B:
Mass of tube + KClO3
6.1029 g
Mass of tube + residue after heating 6.1920 g
Initial gas level in buret (mL) 44.5 mL
Final gas level in buret (mL) 49.7 mL
Room Temperature ( C °) 22.6°C
Barometric Pressure mm Hg) ( 710.0 …show more content…
We were able to determine the moles of a gas which resulted to 5.5x〖10〗^(-3)mol O_2. This led to a R constant, 2.1 x 〖10〗^(-2) (atm∙L)/(mol∙K). Graph 1 did not result as linear as expected but it did have a negative slope to an extant which demonstrated that as the volume gets higher then the pressure decreases. Graph 2 and 3 did have a more positive slope proving that as the pressure increases, the 1/V and PV also increased. The graphs do not appear to be straight lines as Boyle’s law states meaning our results had errors that did not strengthen or support the law but it did demonstrate that they can have a relationship just proper instructions need to be followed.
Conclusion
In conclusion, determining constant was not as easy as assumed with just one wrong number it can change the direction of graphs and misinterpret if PV have a relationship. This experiment did have unavoidable errors such as both gross and systematic errors. The equipment used in this experiment was not as accurate as the ones needed and also the technique used could not be as précised. One may try to avoid errors by continuing with more determinations.