A balloon has a volume of 2.75 liters at 25 degrees celsius. What would the balloon's volume be if the temperature is raised to 95 degrees celsius and the pressure remains constant?

(V1/T1) = (V2/T2)

0.0012

To solve this problem, we need to use Charles's Law, which states that the volume of a gas is directly proportional to its temperature, assuming the pressure remains constant.

Charles's Law can be represented by the formula:
V1/T1 = V2/T2

Where:
V1 = initial volume
T1 = initial temperature in Kelvin
V2 = final volume (what we want to find)
T2 = final temperature in Kelvin

First, let's convert the initial temperature given in degrees Celsius to Kelvin. The Kelvin temperature scale is used in gas laws because it starts from absolute zero (0 K).

To convert from Celsius to Kelvin, we use the formula:
T(K) = T(°C) + 273.15

Given that the initial temperature (T1) is 25 degrees Celsius, we can convert it to Kelvin:
T1 = 25 + 273.15 = 298.15 K

Now we can use Charles's Law to find the final volume (V2) at a temperature of 95 degrees Celsius:
V1/T1 = V2/T2

Substituting the values we have:
2.75/298.15 = V2/95 + 273.15

Now, we can solve for V2 by rearranging the equation:
V2 = (2.75 * (95 + 273.15)) / 298.15

Calculating this will give us the final volume of the balloon when the temperature is raised to 95 degrees Celsius.