Question

1. A mixture of neon and nitrogen gases, in a 8.00 L flask at 42 °C, contains 3.03 grams of neon and 6.80 grams of nitrogen. The partial pressure of nitrogen in the flask is atm and the total pressure in the flask is atm.( 2answers)

2. A mixture of krypton and argon gases is maintained in a 8.85 L flask at a pressure of 3.89 atm and a temperature of 24 °C. If the gas mixture contains 71.5 grams of krypton, the number of grams of argon in the mixture is g.

3. The stopcock connecting a 3.47 L bulb containing argon gas at a pressure of 8.51 atm, and a 2.73 L bulb containing methane gas at a pressure of 3.10 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is atm.

Answer 1

1)

Molar mass of N2 = 28.02 g/mol

mass(N2)= 6.80 g

use:

number of mol of N2,

n = mass of N2/molar mass of N2

=(6.8 g)/(28.02 g/mol)

= 0.2427 mol

Given:

V = 8.0 L

n = 0.2427 mol

T = 42.0 oC

= (42.0+273) K

= 315 K

use:

P * V = n*R*T

P * 8 L = 0.2427 mol* 0.08206 atm.L/mol.K * 315 K

P = 0.784 atm

This is partial pressure for N2

Molar mass of Ne = 20.18 g/mol

mass(Ne)= 3.03 g

use:

number of mol of Ne,

n = mass of Ne/molar mass of Ne

=(3.03 g)/(20.18 g/mol)

= 0.1501 mol

Given:

V = 8.0 L

n = 0.1501 mol

T = 42.0 oC

= (42.0+273) K

= 315 K

use:

P * V = n*R*T

P * 8 L = 0.1501 mol* 0.08206 atm.L/mol.K * 315 K

P = 0.485 atm

This is partial pressure for Ne

Total pressure = 0.784 atm + 0.485 atm = 1.27 atm

partial pressure of N2 = 0.784

Total pressure = 1.27 atm

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