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How hot must you heat 313 mL of gas at 42.4°C for it to expand to 2.6 L?

Answer :

Final answer:

The question can be answered by using Charles's Law which discusses the relationship between temperature and volume of gases at constant pressure. The law's formula V1/T1 = V2/T2 was used with the given initial temperature and volume, as well as the expanded volume, to compute for the required final temperature.

Explanation:

The question is asking us to determine the final temperature of a gas when its volume is increased. This problem can be solved using Charles's Law which states that the volume of a given amount of gas is directly proportional to its absolute temperature if the pressure is held constant.

First, we need to convert the initial temperature from Celsius to Kelvin by adding 273.15 to it, giving us 315.55K. Then we can use Charles' Law formula: V1/T1 = V2/T2. In this case, V1 is 313 mL, T1 is 315.55K (given initial conditions), V2 is 2.6L or 2600mL (the expanded volume).

Plugging these into the formula gives us T2 = V2xT1/V1. Doing the math, we get a value for T2 in Kelvin. Don't forget to convert it back to Celsius by subtracting 273.15 from the Kelvin temperature if needed.

Learn more about Charles's Law here:

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Rewritten by : Brahmana