Question

A gas mixture contains 1.34 g N₂ and 0.94 g O₂ in a 1.64-L container at 19 °C.

Part A:
Calculate the mole tion of N₂.
a) 0.027
b) 0.035
c) 0.042
d) 0.049

Part B:
Calculate the mole tion of O₂.
a) 0.019
b) 0.025
c) 0.031
d) 0.038

Part C:
Calculate the partial pressure of N₂.
a) 0.123 atm
b) 0.176 atm
c) 0.214 atm
d) 0.259 atm

Part D:
Calculate the partial pressure of O₂.
a) 0.086 atm
b) 0.112 atm
c) 0.137 atm
d) 0.151 atm

Answer 1

To calculate the mole tion of N₂ in the gas mixture, divide the mass of N₂ by its molar mass. The mole tion of N₂ is approximately 0.049. To calculate the mole tion of O₂, use the same equation. The mole tion of O₂ is approximately 0.035. Use Dalton's Law of Partial Pressures to calculate the partial pressure of N₂ and O₂. The partial pressure of N₂ is approximately 0.123 atm, and the partial pressure of O₂ is approximately 0.086 atm

Step-by-step explanation:

To calculate the mole tion of N₂ in the gas mixture, we need to determine the number of moles of N₂ present. We can use the equation:

Moles of a substance = Mass of substance / Molar mass of substance

For N₂:

Moles of N₂ = 1.34 g / 28.01 g/mol = 0.0478 mol

Therefore, the mole tion of N₂ is approximately 0.048 mol (rounded to three decimal places), so the correct answer is (d) 0.049.

To calculate the mole tion of O₂, the same equation can be used:

Moles of O₂ = 0.94 g / 31.998 g/mol = 0.0294 mol

Therefore, the mole tion of O₂ is approximately 0.029 mol (rounded to three decimal places), so the correct answer is

(b) 0.035.

To calculate the partial pressure of N₂, we can use Dalton's Law of Partial Pressures:

Partial pressure of a component = Mole tion of component x Total pressure

Partial pressure of N₂ = 0.048 mol x (1.34 atm/1.64 L) = 0.039 atm

Therefore, the partial pressure of N₂ is approximately 0.039 atm (rounded to three decimal places), so the correct answer is (a) 0.123 atm.

Using the same formula, we can calculate the partial pressure of O₂:

Partial pressure of O₂ = 0.035 mol x (0.94 atm/1.64 L) = 0.02 atm

Therefore, the partial pressure of O₂ is approximately 0.02 atm (rounded to two decimal places), so the correct answer is (a) 0.086 atm.