Question

You have a balloon filled with hydrogen gas which keeps it at a

constant pressure, regardless of its volume. The initial volume
of the gas is 736 mL at 15.0 °C. The gas is heated until its
volume is 2.28 L, what is its final temperature in degrees
celsius?

Answer 1

To determine the final temperature of a hydrogen-filled balloon after volume expansion, Charles's Law is applied using provided temperatures converted to Kelvin. After calculation, the temperature is converted back to degrees Celsius. The final temperature in degree Celsius is 619.48 °C.

Step-by-step explanation:

The question involves a hydrogen-filled balloon and a temperature change that causes a change in its volume. To find the final temperature after heating, we can apply Charles's Law, which states that the volume of a gas is directly proportional to its absolute temperature, provided the pressure and the amount of gas remain constant.

To calculate the final temperature in degrees Celsius (°C), we first need to convert all the volumes into the same units and the initial temperature into Kelvin (K):

• Initial volume (V1) = 736 mL = 0.736 L

• Initial temperature (T1) = 15.0 °C = 15.0 + 273.15 = 288.15 K

• Final volume (V2) = 2.28 L

Using Charles's Law, the relationship between the initial and final states can be expressed as V1/T1 = V2/T2. After rearranging to solve for the final temperature (T2), we get T2 = V2 * (T1/V1).

Substituting the values we get:

• T2 = (2.28 L * 288.15 K) / 0.736 L= 892.63 K
• T2= 892.63 K - 273.15 K = 619.48 °C.