Question

3. A 1.20-g sample of dry ice is added to a 755 ml flask containing nitrogen gas at a temperature of 25.0 °C and a pressure of 725 mmHg. The dry ice sublimes (converts from solid to gas), and the mixture returns to 25.0 °C. What is the total pressure in the flask? MISSED THIS? Read Section 6.6; Watch KCV 6.6

Answer 1

We need to use Ideal gas equation to solve this problem. Detailed solution has been attached.

Answer: Total pressure in the flask is 1.84 atm.
we will need to use ideal gas equation to solve this problem. initial pressure of the flash pressure of Nitrogen gas = 725 mm Hg. final pressure of the flash pressure of nitrogens gees + pressure of carbon dioxide Peotal = PN₂ + PCO₂ - 0 PN2 is giun, calculating Peoni PV = nRT Lideal gas equation) Ilco = nRT Peoxen - R = 0.082 6 atm L mole k I 25,0° L-273,15 +2510 = 298.15K Vrained with 55 ml CamScanner = 0.755 l.

na number of moles of co₂ In - giun mass of cor molar mass of cor 0.0273 moles. na 1. 2og ___44.09 Putting values of n, R, I and I in equations Peoz a 0.0273 mole * 0.082.6.atm K_ 298.15K molek 0.755 2 → PCO = 0.88_47 atma P total = PN2 + Por IPN = 725 mm Hg = 0.954 atm 7 p total = 0.95 4 atm t 0.88 47 atm P total = 1.84 atm. Answer Scanned with CamScanner