What is the total pressure when 0.400 g of H2, 2.00 g of N2, and 10.5 g of CO2 are injected into a 10.0 liter flask at 273 K?

0.93 atm is the total pressure for the mixture

Explanation:

In a mixture of gases, we can apply the Ideal Gases Law to determine the total pressure.

Total pressure. V = Total moles. R. T

Let's find out the total moles. Therefore, we must convert the mass to moles:

0.4 g / 2 g/mol = 0.200 mol

2 g / 28g/mol = 0.0714 mol

10.5 g / 44g/mol = 0.238 mol

Total moles = 0.200 + 0.143 + 0.0714 → 0.4144 moles

We replace the data to the formula

Total pressure. 10L = 0.4144 moles. 0.082 L. atm/mol. K. 273K

Total pressure = (0.4144 moles. 0.082 L. atm/mol. K. 273K) / 10L

Total pressure = 0.93 atm