Question

A mixture of gases contains 5.10 g nitrogen gas, 2.83 g of hydrogen gas and 5.17 g of ammonia gas (NH3). If the total pressure of the mixture is 4.21 atm, what is the partial pressure of N2? A 2.77 atm B 0.812 atm C 0.406 atm D 0.575 atm E 0.966 atm

          A mixture of gases contains 5.10 g nitrogen gas, 2.83 g of hydrogen gas and 5.17 g of ammonia gas (NH3). If the total pressure of the mixture is 4.21 atm, what is the partial pressure of N2?
A 2.77 atm
B 0.812 atm
C 0.406 atm
D 0.575 atm
E 0.966 atm

A mixture of gases contains 5.10 g nitrogen gas, 2.83 g of hydrogen gas and 5.17 g of ammonia gas (NH3). If the total pressure of the mixture is 4.21 atm, what is the partial pressure of N2?
A 2.77 atm
B 0.812 atm
C 0.406 atm
D 0.575 atm
E 0.966 atm

Added by Sandy W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

07/25/2023

Step 1

Calculate the total moles of gas in the mixture: - Moles of N2 = 5.10 g / 28.01 g/mol = 0.182 mol - Moles of H2 = 2.83 g / 2.02 g/mol = 1.40 mol - Total moles = 0.182 mol + 1.40 mol = 1.58 mol Show more…

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A mixture of gases contains 5.10 g of nitrogen gas, 2.83 g of hydrogen gas, and 5.17 g of ammonia gas. The total pressure of the mixture is 4.21 atm. What is the partial pressure of N2?