Question

Under constant-pressure conditions a sample of hydrogen gas initially at 53.00°C and 7.10 L is cooled until its final volume is 4.10 L. What is its final temperature?

Answer 1

Using Charles's Law and the given initial conditions of a hydrogen gas sample, the final temperature after cooling to a volume of 4.10 L at constant pressure is determined to be -85.28°C.

Step-by-step explanation:

To determine the final temperature of a sample of hydrogen gas cooled from 53.00°C to a final volume of 4.10 L at constant pressure, we can use Charles's Law. This law states that for a fixed amount of gas at constant pressure, the volume of the gas is directly proportional to its temperature (in Kelvin).

To find the final temperature, we first convert the initial Celsius temperature to Kelvin (T1 = 53 + 273.15 = 326.15 K) and then use the equation:

V1/T1 = V2/T2

Plugging in the initial volume (V1 = 7.10 L), initial temperature (T1 = 326.15 K), and final volume (V2 = 4.10 L), we can solve for the final temperature (T2).

T2 = (V2 × T1) / V1

T2 = (4.10 L × 326.15 K) / 7.10 L

T2 = 187.87 K

To convert back to Celsius: T2 = 187.87 K - 273.15 = -85.28°C

Therefore, the final temperature of the hydrogen gas is -85.28°C.