Question

Use Charles's Law to solve the following problem. A sample of air has a volume of 550.0 mL at 106 °C. At what temperature will its volume be 700.0 mL at constant pressure?

a. 482 K
b. 63 °C
c. 505 K
d. 119 °C

Answer 1

Using Charles's Law and converting the initial temperature to Kelvin, the final temperature when the gas volume increases to 700.0 mL was calculated to be approximately 482 K, which corresponds to answer choice (a).

Step-by-step explanation:

To solve the problem using Charles's Law, we first convert the initial temperature from Celsius to Kelvin since gas laws require temperatures to be in Kelvin. Therefore, 106 °C + 273 = 379 K. Charles's Law states that at constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin. That is, V1/T1 = V2/T2.

We can rearrange this to solve for T2: T2 = (V2 × T1) / V1. Plugging in values we have T2 = (700.0 mL × 379 K) / 550.0 mL. Simplifying, we get T2 = 481.818 K, which when rounding to an integer is approximately 482 K.

Thus, the final answer is 482 K, which corresponds to choice (a).