Question

Which of the following temperature changes would cause a fixed amount of gas at constant pressure to double in volume? a. decrease from 60°c to 30°c b. increase from 20°c to 40°c c. decrease from 400 k to 200 k d. increase from 150 k to 300 k

Answer 1

The temperature change that would cause a fixed amount of gas at constant pressure to double in volume, according to Charles' Law, is an increase from 150 K to 300 K

Step-by-step explanation:

The behavior of gases under varying temperature, volume, and pressure conditions can be predicted with the ideal gas law, which states PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin (K). Here, we're given a fixed amount of gas at constant pressure, so we're essentially looking at the relationship between volume (V) and temperature (T).

When temperature doubles in Kelvin scale (since it's the absolute temperature scale), the volume should double as well according to Charles' Law. Therefore, the correct answer to the question is d. increase from 150 K to 300 K. It's only in this option where temperature precisely doubles, assuming the levels given are in Kelvin (the absolute temperature scale required by the gas laws).

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