Solution Found!
Liquid nitrogen trichloride is heated in a 2.50-L closed
Chapter 6, Problem 82P(choose chapter or problem)
Liquid nitrogen trichloride is heated in a 2.50-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 754 mmHg at 95°C. (a) What is the partial pressure of each gas in the container? (b) What is the mass of the original sample?
Questions & Answers
QUESTION: Problem 82P
Liquid nitrogen trichloride is heated in a 2.50-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 754 mmHg at 95°C. (a) What is the partial pressure of each gas in the container? (b) What is the mass of the original sample?
ANSWER:
Solution 82P
Here we have to calculate the partial pressure of each gas present in the container
Containing liquid nitrogen trichloride and have to find out the mass of the original sample.
Step 1
(a) Calculation of partial pressure of each gas:-
Given:
Volume of the vessel = 2.50 L
Pressure = 754 mm Hg= 754/760 = 0.992 atm
Temperature = 95oC = 273 + 95 = 368 K
The balanced chemical equation for the decomposition of liquid nitrogen chloride is given below,
2NCl3 (l) → N2(g) + 3Cl2 (g)
The partial pressure of N2 can be calculated as follows,
=
P
Where =
and P is the pressure
Now substituting the values,
=
754 mm Hg
= 188.5 mm Hg
The partial pressure of Cl2 can be calculated as follows,
=
P
Where =
and P is the pressure
Now substituting the values,
=
754 mm Hg
= 565.5 mm Hg
Thus the partial pressure of N2 gas is found to be 188.5 mm Hg and the partial pressure of Cl2 is found to be 565.5 mm Hg.