What is the total pressure in units of kPa in a 7.85 L container that contains 4.45 moles of N2 and 2.45 moles of O2 at a temperature of 307 K?

Total pressure = 22.15 atm

Explanation:

Given data:

Total pressure = ?

Volume of container = 7.85 L

Number of moles of N₂ = 4.45 mol

Number of moles of O₂ = 2.45 mol

Temperature = 307 K

Solution:

Pressure of N₂:

PV = nRT

P = nRT/V

P = 4.45 mol ×0.0821 atm.L/mol.K ×307K / 7.85L

P = 112.16 atm.L/7.85 L

P = 14.28 atm

Pressure of O₂:

PV = nRT

P = nRT/V

P = 2.45 mol ×0.0821 atm.L/mol.K ×307K / 7.85L

P = 61.75 atm.L/7.85 L

P = 7.87 atm

Total pressure = P(N₂) + P(O₂)

Total pressure = P( 14.28 atm)  +  P( 7.87 atm)

Total pressure = 22.15 atm

a basic solution is an aqueous solution containing more oh-ions than h+ions. in other words, it is an aqueous solution with a ph greater than 7. basic solutions contain ions, conduct electricity, turn red litmus paper blue, and feel slippery to the touch.

explanation: