Final answer:
The volume of a helium balloon containing 2.50 mol of helium at 27°C and 1.10 atm can be calculated using the ideal gas law. With the temperature converted to Kelvin and applying the known values, one can find the volume by the formula V = nRT/P.
Step-by-step explanation:
The volume of a helium balloon containing 2.50 mol of helium at 27°C and 1.10 atm can be determined using the ideal gas law, which is PV = nRT. Here P represents pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant (0.0821 L·atm·K⁻¹·mol⁻¹), and T is the temperature in Kelvin. First, convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. Thus, 27°C is equal to 300.15 K.
To find the volume, rearrange the ideal gas law formula to V = nRT/P. By plugging in the known values: V = (2.50 mol)(0.0821 L·atm·K⁻¹·mol⁻¹)(300.15 K) / (1.10 atm), we can calculate the volume of the balloon.