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At 27°C, a 250 mL sample of gas was expanded to 375 mL at constant pressure. What is the new temperature of the gas?

Answer :

Final answer:

The final temperature of the gas, given the initial conditions and the application of Charles's Law, is approximately 177.075°C or 450.225K.

Explanation:

Your question involves the application of Charles's Law which states that the volume of gas is directly proportional to its temperature under constant pressure. This principle is used frequently in Physics and Chemistry.

To determine the new temperature of the gas, we use the equation based on Charles's Law: V1/T1 = V2/T2. In this case, V1 = 250 mL, T1 = 27°C (which is 300.15K in Kelvin), and V2 = 375 mL. We are asked to find T2.

First, we rearrange the equation to solve for T2: T2 = V2 * T1 / V1. Substituting the given values into the equation yields: T2 = 375 mL * 300.15 K / 250 mL = 450.225 K.

The temperature in Kelvin might be more helpful, but if you need the temperature in degrees Celsius, remember that you subtract 273.15 from the Kelvin temperature: 450.225 - 273.15 = 177.075°C.

Learn more about Charles's Law here:

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