If a student increases the temperature of a balloon from 30°C to 50°C, assuming constant pressure, what will happen to the volume of the balloon?
To understand what will happen to the volume of the balloon when the temperature increases, we can use the ideal gas law, which states:
PV = nRT
Where:
P = pressure of the gas,
V = volume of the gas,
n = number of moles of gas,
R = ideal gas constant (8.314 J/(mol·K)),
T = temperature of the gas in Kelvin.
In this case, we can assume the pressure remains constant, so we can rewrite the equation as:
V₁ / T₁ = V₂ / T₂
Where:
V₁ = initial volume of the balloon,
T₁ = initial temperature (in Kelvin),
V₂ = final volume of the balloon,
T₂ = final temperature (in Kelvin).
To solve the problem, we need to convert the temperatures from Celsius to Kelvin:
T₁ = 30°C + 273.15 = 303.15 K
T₂ = 50°C + 273.15 = 323.15 K
Now we can use the formula:
V₁ / 303.15 K = V₂ / 323.15 K
Now we can solve for V₂:
V₂ = (V₁ / 303.15 K) * 323.15 K
Therefore, we can see that increasing the temperature from 30°C to 50°C will cause an increase in the volume of the balloon, assuming constant pressure.