Question

A 2.50‑liter volume of hydrogen measured at –196 °C is warmed to 100 °C. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.

A) 12.1 L
B) 1.28 L
C) 4.9 L
D) 0.517 L

Answer 1

The volume of the gas at the higher temperature is 12.1 L.

Step-by-step explanation:

Charles's Law:

Charles's Law states that the volume of a gas at constant pressure is directly proportional to its temperature. Mathematically, it can be expressed as:

V1/T1 = V2/T2

where:

V1 is the initial volume

T1 is the initial temperature in Kelvin

V2 is the final volume

T2 is the final temperature in Kelvin

Convert temperatures to Kelvin:

Initial temperature (T1) = -196°C + 273.15 = 77.15 K

Final temperature (T2) = 100°C + 273.15 = 373.15 K

Apply Charles's Law:

V1 = 2.50 L

T1 = 77.15 K

V2 = unknown

T2 = 373.15 K

Substitute the values into the equation:

2.50 L / 77.15 K = V2 / 373.15 K

Solve for V2:

V2 = 2.50 L * 373.15 K / 77.15 K

V2 ≈ 12.1 L

Therefore, the volume of the gas at 100°C is 12.1 L.