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A sample of oxygen gas initially at 375 K was heated to 429 K. If the volume of the oxygen gas sample at 429 K is 836.5 mL, what was its volume at 375 K?

A) 836.5 mL
B) 723.6 mL
C) 680.9 mL
D) 792.1 mL

Answer :

Final Answer:

It represents the calculated initial volume of the oxygen gas sample at 375 K based on the application of Charles's Law. Therefore the correct option is B) 723.6 mL

Explanation:

When a gas is heated at constant pressure, its volume is directly proportional to its absolute temperature, as described by Charles's Law. The formula for Charles's Law is V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature, respectively.

Given:

Initial temperature (T1) = 375 K

Final temperature (T2) = 429 K

Final volume (V2) = 836.5 mL

We need to find the initial volume (V1) at 375 K.

Using Charles's Law:

V1/T1 = V2/T2

V1/375 = 836.5/429

Now, solve for V1:

V1 = (836.5 * 375) / 429

V1 ≈ 723.6 mL

So, the initial volume of the oxygen gas sample at 375 K is approximately 723.6 mL.

Charles's Law states that the volume of a gas is directly proportional to its absolute temperature when the pressure and the amount of gas are held constant. In this problem, we are given the initial and final temperatures and the final volume of the oxygen gas sample. We can use Charles's Law to find the initial volume by setting up a proportion and solving for V1.

To do this, we plug in the known values: T1 (initial temperature) = 375 K, T2 (final temperature) = 429 K, and V2 (final volume) = 836.5 mL. Solving for V1, we find that the initial volume is approximately 723.6 mL.

This result makes sense because as the temperature of a gas increases, its volume also increases, assuming the pressure and the amount of gas remain constant. The initial volume is less than the final volume, as the gas was initially at a lower temperature.

Therefore the correct option is B) 723.6 mL

Learn more about Charles's Law

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