Answer:
Initial pressure of N2 was 413 torr
Explanation:
Given:
- Initial Pressure of H2 = 353 torr
- Initial Volume of H2 = 2 L
- Final Volume of H2 = 3 L
- Total pressure at end = 373 torr
- Iinitial Volume of N2 = 1 L
- Final Volume of N2 = 3 L
Find:
determine the initial pressure of N2 in the 1.00 L flask.
Solution:
- Lets focus on the H2 at first, from pascal's Law we have:
P_1 x V_1 = P_2 x V_2
(353)(2) = (P)(3)
P = 353*2 / 3 = 235.333 torr
- Since the total pressure remains constant the Pressure P of the N2 at the end would be
373 - 235.33 = 137.667 torr
- Now calculate the original P of N2 , again using Pascal's Law:
(P)(1) = (137.667)(3)
P = 137.667*3 = 413 torr
Answer: Initial pressure of N2 was 413 torr
This question involves the concepts of Boyle's Law and Dalton's Law of Partial Pressure.
The initial pressure of N₂ in 1 L flask was "413 torr".
First, we will calculate the final volume of H₂ by using Boyle's Law:
[tex]P_1V_1=P_2V_2\\\\P_2=\frac{P_1V_1}{V_2}[/tex]
where,
P₁ = initial pressure of H₂ = 353 torr
V₁ = initial volume of H₂ = 2 L
V₂ = final volume of H₂ = 3 L
P₂ = final pressure of H₂ = ?
Therefore,
[tex]P_2=\frac{(353\ torr)(2\ L)}{3\ L}\\\\[/tex]
P₂ = 235.33 torr
Now, we will use Dalton's Law of Partial Pressure to find ut the final pressure of N₂:
Total Final Pressure = Final Pressure of H₂ + Final Pressure of N₂
Final Pressure of N₂ = 373 torr - 235.33 torr
Final Pressure of N₂ = 137.67 torr
Now, we will again use Boyle's Law for N₂ to find out the initial pressure of N₂:
[tex]P_1V_1=P_2V_2\\\\P_1=\frac{P_2V_2}{V_1}[/tex]
where,
P₁ = initial pressure of N₂ = ?
V₁ = initial volume of N₂ = 1 L
V₂ = final volume of N₂ = 3 L
P₂ = final pressure of N₂ = 137.67 torr
Therefore,
[tex]P_1=\frac{(137.67\ torr)(3\ L)}{1\ L}\\\\[/tex]
P₁ = 413 torr
Learn more about Boyle's Law here:
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