7. -13 points The density of a noble gas is 0.536 g/L at 3.00 atm and 0°C. Ident

Question

7. -13 points The density of a noble gas is 0.536 g/L at 3.00 atm and 0°C. Identify the gas. 8. -14 points My Notes When 0.677 L of Ar at 1.20 atm and 227°C is mixed with 0.272 L of O2 at 501 torr and 127°C in a 400. mL flask at 27°C, what is the pressure in the flask? atm 9. -13 points FOLLOW-UP PROBLEM 5.9 Applying Dalton's Law of Partial Pressures To prevent the presence of air, noble gases are placed over highly reactive chemicals to act as inert "blanketing" gases. A chemical engineer places a mixture of noble gases consisting of 6.01 g of He, 15.0 g of Ne, and 35.1 g of Kr in a piston-cylinder assembly at STP. Calculate the partial pressure of each gas. HINTS atm atm atm Getting Started

Explanation / Answer

7)
P = 3.0atm
T= 0.0 oC
= (0.0+273) K
= 273 K
density = 0.536 g/L
Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T

Put Values:
3.0 atm * MM = density * 0.0821 atm.L/mol.K *273.0 K
MM = 4.0045 g/mol

This is molar mass of Helium
Answer: Helium

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