Question

At standard temperature, a gas has a volume

of 368 mL. The temperature is then increased
to 137◦C, and the pressure is held constant.
What is the new volume?
Answer in units of mL.

Answer 1

Using Charles's Law, the new volume of a gas when its temperature is increased to 137°C while maintaining constant pressure is found to be 522.4 mL after converting temperatures to Kelvin and applying the law's formula.

Step-by-step explanation:

The student's question involves finding the new volume of a gas when the temperature is increased, while the pressure is held constant. This situation is described by Charles's Law, which states that the volume of a gas is directly proportional to its temperature as long as the pressure and the amount of gas remain constant. The temperature must be in Kelvin for this calculation.

First, we convert the initial temperature from degrees Celsius to Kelvin. The initial temperature in Kelvin is 14.0 °C + 273.15 = 287.15 K. Next, the final temperature is also converted to Kelvin: 137 °C + 273.15 = 410.15 K.

Then, we use Charles's Law in the form of V1/T1 = V2/T2. After plugging in our known values, we can solve for V2, which gives us the new volume of the gas.

Applying Charles's Law:

368 mL / 287.15 K = V2 / 410.15 K
V2 = 368 mL * (410.15 K / 287.15 K)
V2 = 522.4 mL

Therefore, the new volume of the gas when the temperature is increased to 137°C at constant pressure is 522.4 mL.