What mass of helium would be contained within a 1.8 L balloon at a pressure of 766 torr and a temperature of 24.5°C?

Question

Quizplus · Accepted Answer

To find the mass of helium in the balloon, 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, R is the ideal gas constant, and T is the temperature in Kelvin. First, convert the given values to the appropriate units: pressure in atm (766 torr / 760 torr/atm = 1.0079 atm), volume in liters (already given as 1.8 L), and temperature in Kelvin (24.5°C + 273.15 = 297.65 K). Using R = 0.0821 L·atm/(mol·K), solve for n (moles of helium). Then, multiply the number of moles by the molar mass of helium (about 4.00 g/mol) to find the mass. The calculation leads to a mass close to 0.297 g, making option B correct.

What Mass of Helium Would Be Contained Within a 1