A balloon has a volume of 2.75 liters at 25 degree celcus. What would the balloons volume be if the temperature is raised to 95 degree celcus and the pressure remains constant?
please provide steps to get to answer
V1/T1 = V1/T2
Don't forget to change T to Kelvin.
Also, note the correct spelling of celsius.
I made a typo. The equation should be
V1/T1 = V2/T2
To solve this problem, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin.
To find the new volume of the balloon when the temperature is raised to 95 degrees Celsius, we need to convert the temperatures from Celsius to Kelvin:
Step 1: Convert temperature from Celsius to Kelvin
- Add 273.15 to the given temperatures.
- The initial temperature is 25 degrees Celsius + 273.15 = 298.15 Kelvin.
- The new temperature is 95 degrees Celsius + 273.15 = 368.15 Kelvin.
Step 2: Set up the equation and solve for the new volume
- Since the pressure remains constant, we can rewrite the equation as V₁/T₁ = V₂/T₂, where V₁ is the initial volume, T₁ is the initial temperature in Kelvin, V₂ is the new volume (to be found), and T₂ is the new temperature in Kelvin.
- Plugging in the values: 2.75 L / 298.15 K = V₂ / 368.15 K.
- Cross-multiply and solve for V₂: 2.75 L * 368.15 K = V₂ * 298.15 K.
- Divide both sides by 298.15 K to isolate V₂: V₂ = (2.75 L * 368.15 K) / 298.15 K.
- Calculate: V₂ ≈ 3.39 L.
Therefore, the volume of the balloon would be approximately 3.39 liters if the temperature is raised to 95 degrees Celsius while the pressure remains constant.