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

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm