Question

To what temperature must a balloon, initially at 25°C and 2.00 L, be heated in order to have a volume of 6.00 L?

A) 993 K
B) 403 K
C) 75 K
D) 655 K
E) 894 K

Answer 1

Using Charles's Law and converting Celsius to Kelvin, the final temperature needed to increase the balloon's volume to 6.00 L is approximately 894 K, corresponding to answer choice E.

Step-by-step explanation:

To solve this problem, we can use Charles's Law, which states that if the pressure of a gas is constant, its volume is directly proportional to its absolute temperature (in Kelvin). The formula for Charles's Law is V1/T1 = V2/T2, where V1 and T1 are the initial volume and temperature, and V2 and T2 are the final volume and temperature.

First, we need to convert the initial temperature from Celsius to Kelvin. We do this by adding 273.15 to the Celsius temperature:

T1 = 25°C + 273.15 = 298.15 K

Now we can set up the equation with the known values:

(2.00 L / 298.15 K) = (6.00 L / T2)

To solve for T2, we cross-multiply and divide:

T2 = (6.00 L * 298.15 K) / 2.00 L

T2 = 894.45 K

After calculating, we find that the temperature T2 must be approximately 894 K to increase the volume of the balloon to 6.00 L, which corresponds to answer choice E (894 K).