Question

If you had a balloon with a volume of 1463 ml and a temperature of 80°C, what temperature in °C would you need to change it to if you wanted the balloon to have a volume of 1.13 liters?

A) 100°C
B) 200°C
C) 300°C
D) 400°C

Answer 1

Using Charles's Law, the temperature needed to change the balloon with a volume of 1463 ml at 80°C to a volume of 1.13 liters is approximately 2.4°C. This result is not found among the provided multiple-choice options, suggesting a potential error in the provided data.

Step-by-step explanation:

To solve this question, we can apply Charles's Law, which states that the volume of a gas is directly proportional to its temperature when pressure is held constant. Given this, we use the formula V1/T1 = V2/T2 where V1 and T1 are the initial volume and temperature of the gas, and V2 and T2 are the final volume and temperature, respectively. We must remember to convert all temperatures to Kelvin by adding 273 to the Celsius value. Since the question requires temperature to remain in Celsius, we'll convert it back to Celsius after our calculation.

Starting with the initial conditions: V1 = 1463 mL or 1.463 liters, T1 = 80°C or 353 K, we want to find the temperature at a new volume of V2 = 1.13 liters.

To find T2, we rearrange the above formula to T2 = (V2 * T1) / V1. When we plug in our values:

T2 = (1.13 L * 353 K) / 1.463 L = 275.4 K.

Converting back to Celsius: T2 = 275.4 K - 273 = 2.4°C.

This answer is not listed in the options A through D, indicating there might be a mistake in the question or the multiple-choice options provided. Based on the calculation using Charles's Law, a temperature change to approximately 2.4°C would cause the balloon to have a volume of 1.13 liters under constant pressure.