A glass laboratory flask is filled with gas at 24 ∘C and 0.95 atm pressure, sealed, and then heated to 104 ∘C. What is the pressure inside the flask?

The pressure inside the flask on heating it is given as 1.21 atm.

Explanation:

As per Guy Lussac's law, the pressure of any concealed volume of gas particles will be directly proportional to the temperature of the container of the gas particles.

So P ∝ T

To convert celsius to kelvin, add 273.15 to the temperature value in celsius

Since, here the initial temperature of the flask is given as 24°C, so in kelvin it will be 297.15 K. Similarly, the final temperature is said to be 104°C which will be equal to 377.15 K. Then the final pressure will be increased as there is increase in temperature. So, the final pressure inside the flask can be obtained as

So, the pressure inside the flask on heating it is given as 1.21 atm.

Final answer:

Using Gay-Lussac's law, the final pressure of the gas in the flask after heating from 24°C to 104°C, under a constant volume, is approximately 1.2 atm.

Explanation:

The pressure inside the flask can be calculated by using Gay-Lussac's law, which states that the pressure of a gas is directly proportional to its absolute temperature, as long as volume is constant. This is formally expressed as P1/T1 = P2/T2, where P is pressure, T is absolute temperature (in Kelvin), and the subscripts refer to initial and final states.

First, convert the Celsius temperatures to Kelvin by adding 273.15 to the Celsius temperature. T1 = 24°C + 273.15 = 297.15 K, and T2 = 104°C + 273.15 = 377.15 K. Next, rearrange the equation to solve for P2: P2 = P1 (T2 / T1).

So, P2 = 0.95 atm * (377.15 K / 297.15 K) ≈ 1.2 atm. Therefore, the pressure inside the glass laboratory flask after heating to 104°C would be approximately 1.2 atm.

Learn more about Gay-Lussac's law here:

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