An air bubble has a volume of 0.500 L at 26 Celsius.
If the pressure does not change, what is the volume, in liters, at -14 Celsius?
If the pressure does not change, what is the volume, in liters, at 600 k?
V1/T1 = V2/T2
T1 and T2 must be in Kelvin.
To solve these problems, we can use Charles's Law, which states that the volume of a fixed amount of gas is directly proportional to its temperature, assuming that pressure remains constant.
To find the initial volume of the air bubble, given the temperature of 26 °C, we can use the formula:
V1 / T1 = V2 / T2
Where:
V1 = initial volume
T1 = initial temperature
V2 = final volume
T2 = final temperature
Let's solve the first problem:
Given:
V1 = 0.500 L
T1 = 26 °C
T2 = -14 °C
Using the formula, we have:
0.500 L / (26 + 273) K = V2 / (-14 + 273) K
Converting temperature from Celsius to Kelvin by adding 273:
0.500 L / 299 K = V2 / 259 K
Cross-multiplying, we get:
0.500 L * 259 K = 299 K * V2
Simplifying the equation:
V2 = (0.500 L * 259 K) / 299 K
V2 = 0.433 L
Therefore, the volume of the air bubble at -14°C would be approximately 0.433 liters.
Now let's solve the second problem:
Given:
V1 = 0.500 L
T1 = 26 °C
T2 = 600 K
Using the same formula:
0.500 L / (26 + 273) K = V2 / 600 K
Converting temperature from Celsius to Kelvin by adding 273:
0.500 L / 299 K = V2 / 600 K
Cross-multiplying, we get:
0.500 L * 600 K = 299 K * V2
Simplifying the equation:
V2 = (0.500 L * 600 K) / 299 K
V2 = 1.003 L
Therefore, the volume of the air bubble at 600 K would be approximately 1.003 liters.