Liquid nitrogen trichloride is heated in a 1.25−L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 839 mmHg at 104°C. What is the partial pressure of each gas in the container?

The partial pressure of N2 is 209.75 mmHg

The partial pressure of Cl2 = 629.25 mmHg

Explanation:

Step 1: Data given

Volume of the vessel = 1.25 L

Pressure 839 mmHg = 839/760 atm = 1.10395 atm

Temperature = 104 °C = 377 K

Step 2: The balanced equation

2 NCl3 → N2 + 3 Cl2

For 2 moles NCl3 we'll have 1 mol N2 and 3 moles Cl2

Step 3: Calculate partial pressure

partial pressure Cl2 = 3 x partial pressure N2

partial pressure N2 + 3 x partial pressure N2 = 839

x + 3x = 839

x = 209.75 mm Hg = partial pressure N2

partial pressure Cl2 = 3x = 629.25 mm Hg

The partial pressure of N2 is 209.75 mmHg

The partial pressure of Cl2 = 629.25 mmHg

the atomic mass is the bottom number on the element.

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