Pls help
1. Determine the new pressure when the constant volume of gas at 1.00atm is heated from 20.0°C to 30.0°C.
2. If 23.1 g of O₂ occupies a volume of 5.0L at a particular temperature and pressure what volume will 2.50g of oxygen gas occupy under the same conditions?
3. At conditions of 785.0 torr and 15.0°C, a gas occupies a volume of 45.5 ml, what will be the volume of the same gas at 745.0 torr and 30.0°C?
I would really appreciate it if you answer this thank you :)
1. Determine the new pressure when the constant volume of gas at 1.00atm is heated from 20.0°C to 30.0°C.
2. If 23.1 g of O₂ occupies a volume of 5.0L at a particular temperature and pressure what volume will 2.50g of oxygen gas occupy under the same conditions?
3. At conditions of 785.0 torr and 15.0°C, a gas occupies a volume of 45.5 ml, what will be the volume of the same gas at 745.0 torr and 30.0°C?
I would really appreciate it if you answer this thank you :)
Answers & Comments
Answer:
1. Pressure of a gas at constant volume is directly proportional to its temperature (in Kelvin) according to the ideal gas law. So, the pressure after heating the gas from 20.0°C to 30.0°C would be 1.00atm * (303.15K / 293.15K) = 1.03atm.
2. According to the Ideal gas law, the volume of a gas is proportional to the number of moles it contains. The number of moles of O₂ in 23.1 g is (23.1g) / (32.00 g/mol) = 0.722 mol, and in 2.50g is (2.50g) / (32.00 g/mol) = 0.078125 mol. So, the volume occupied by 2.50 g of O₂ would be 5.0 L * (0.078125 mol) / (0.722 mol) = 0.525 L.
3. According to Boyle's Law, the volume of a gas is inversely proportional to its pressure at constant temperature. The volume occupied by the gas at 745.0 torr and 30.0°C would be 45.5 ml * (785.0 torr) / (745.0 torr) = 48.1 ml.