Question

A mixture of gases contains 2.14 g of N2, 5.85 g of H2, and 18.58 g of NH3. If the total pressure of the mixture is 4.58 atm, what is the partial pressure of NH3? Hint: Determine the mole fraction of NH3 first and then multiply that ratio by the total pressure.

Name: a mixture of gases contains 214 g of n2 585 g of h2 and 1858 g of nh3 if the total pressure of the mixture is 458 atm what is the partial pressure of nh3 hint determine the mole fraction of 60912
Uploaded: 2023-08-14T09:52:24-08:00
Duration: 2 min 31 s
Channel: Madhur L
Description: a mixture of gases contains 214 g of n2 585 g of h2 and 1858 g of nh3 if the total pressure of the mixture is 458 atm what is the partial pressure of nh3 hint determine the mole fraction of 60912

          A mixture of gases contains 2.14 g of N2, 5.85 g of
H2, and 18.58 g of NH3. If the total pressure
of the mixture is 4.58 atm, what is the partial pressure of
NH3?
Hint: Determine the mole fraction of
NH3 first and then multiply that ratio by the total
pressure.

Added by Amy C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

08/14/2023

Step 1

Moles of N2 = mass / molar mass = 2.14 g / 28.02 g/mol = 0.0763 mol Moles of H2 = mass / molar mass = 5.85 g / 2.02 g/mol = 2.896 mol Moles of NH3 = mass / molar mass = 18.58 g / 17.03 g/mol = 1.091 mol Show more…

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A mixture of gases contains 2.14 g of N2, 5.85 g of H2, and 18.58 g of NH3. If the total pressure of the mixture is 4.58 atm, what is the partial pressure of NH3? Hint: Determine the mole fraction of NH3 first and then multiply that ratio by the total pressure.