Sorry, I know that this problem might not be as complicated asit sounds. But my

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Sorry, I know that this problem might not be as complicated asit sounds. But my brain is stuck after studying too much from myother exams that I can't think properly anymore. In the laboratory, you will test Charles's Law using a syringefilled with air. Because of the movable plunger on the syringe, thegas inside the syringe can be held at a constant pressure of 1.00atm while allowing the volume of the gas to increase ordecrease. a) You fill a syringe with 5.0ml of air at 25oC and1.00atm. How many moles of air are contained in the syringe? b) Assuming that the mole fraction of nitrogen in air is 0.79and the mole fraction of oxygen in air is 0.21, determine thepartial pressure of each gas, and the mass of each gas contained inthe syringe. c) On repeating the expreiment, you accidentally trap a smallamount of water inside the syringe. (Assume that the water vapporreaches equilibrium inside the syringe, and neglect the volume ofthe liquid water which will be present.) Given atemperature of 25oC, a volume of 5.0 mL, and atotal pressure of 1.00atm, determine the partial pressureof water vapor and the partial pressure of air (without watervapor) inside the syringe. d) You increase the tempreature of the syringe to65oC; the total pressure remains 1.00 atm, but thevolume increases. Determine the volume of the syringe at the newtemperature (Assume that the water vapor reaches equilibrium at65oC). Thank you very much in advance. And sorry for the long work. Ihope you understand my situation. Thank you. Sorry, I know that this problem might not be as complicated asit sounds. But my brain is stuck after studying too much from myother exams that I can't think properly anymore. In the laboratory, you will test Charles's Law using a syringefilled with air. Because of the movable plunger on the syringe, thegas inside the syringe can be held at a constant pressure of 1.00atm while allowing the volume of the gas to increase ordecrease. a) You fill a syringe with 5.0ml of air at 25oC and1.00atm. How many moles of air are contained in the syringe? b) Assuming that the mole fraction of nitrogen in air is 0.79and the mole fraction of oxygen in air is 0.21, determine thepartial pressure of each gas, and the mass of each gas contained inthe syringe. c) On repeating the expreiment, you accidentally trap a smallamount of water inside the syringe. (Assume that the water vapporreaches equilibrium inside the syringe, and neglect the volume ofthe liquid water which will be present.) Given atemperature of 25oC, a volume of 5.0 mL, and atotal pressure of 1.00atm, determine the partial pressureof water vapor and the partial pressure of air (without watervapor) inside the syringe. d) You increase the tempreature of the syringe to65oC; the total pressure remains 1.00 atm, but thevolume increases. Determine the volume of the syringe at the newtemperature (Assume that the water vapor reaches equilibrium at65oC). Thank you very much in advance. And sorry for the long work. Ihope you understand my situation. Thank you.

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