Question

A container containing 8.00 L of a gas is collected at 55 K and then allowed to expand to 24.0 L. What must the new temperature be in order to maintain the same pressure? Draw particle diagrams to support your answer.

Answer 1

To maintain the same pressure after a gas expands from 8.00 L at 55 K to 24.0 L, according to Charles's Law, the new temperature must be 165.0 K.

Step-by-step explanation:

The question concerns gas laws, specifically Charles's Law, which states that for a given mass of an ideal gas at constant pressure, the volume is directly proportional to the absolute temperature (in kelvins). Using this law, we can find the new temperature after the expansion of a gas that maintains the same pressure. The initial conditions are 8.00 L at 55 K, and after expansion, the volume is 24.0 L. Applying Charles's Law (V1/T1 = V2/T2), we can calculate the new temperature (T2).

Let's set up the equation with the given values:

• V1 = 8.00 L
• T1 = 55 K
• V2 = 24.0 L
• T2 = unknown

We can solve for T2 as follows:

V1/T1 = V2/T2

8.00 L / 55 K = 24.0 L / T2

T2 = (24.0 L * 55 K) / 8.00 L

T2 = 165.0 K

To maintain the same pressure after the gas expands to 24.0 L, the temperature must be increased to 165.0 K.