If 12g nitrogen gas,0.40 of H2 gas and 9.0 gram of oxygen are put into 1 litre container of. 27°C what is the total pressure on the container?

Total pressure = 27.35 atm

Explanation:

Given data:

Mass of nitrogen = 12 g

Mass of H₂ = 0.40 mol

Mass of oxygen = 9.0 g

Volume of Container = 1 L

Temperature = 27 °C (27+273 = 300 K)

Total Pressure = ?

Solution:

First of all we will calculate the number of moles of individual gas.

Number of moles = mass/ molar mass

Number of moles = 12 g/ 28 g/mol

Number of moles = 0.43 mol

Pressure of N₂:

PV = nRT

P = nRT/V

P = 0.43 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L

P = 10.6 atm

Number of moles of Oxygen:

Number of moles = mass/ molar mass

Number of moles = 9 g/ 32 g/mol

Number of moles = 0.28 mol

Pressure of O₂:

PV = nRT

P = nRT/V

P = 0.28 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L

P = 6.9 atm

Pressure of H₂:

PV = nRT

P = nRT/V

P = 0.40 mol × 0.0821 atm.L/mol.K× 300 K/ 1 L

P = 9.85 atm

Total pressure:

Total pressure = Pressure of H₂ + Pressure of O₂ + Pressure of N₂

Total pressure = 9.85 atm + 6.9 atm + 10.6 atm

Total pressure = 27.35 atm

c u c l 2 + 2 n a n o 3 → c u ( n o 3 ) 2 + 2 n a c l

  long weird answer but i hope this works