50 L container at 305 K holds a 0.22 g sample of carbon dioxide gas (CO₂). Assuming ideal gas behavior, what is the pressure, in kilopascals, exerted by the gas?

Question

Quizplus · Accepted Answer

To find the pressure exerted by the gas, 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 ideal gas constant, and T is the temperature in Kelvin. First, we need to convert the mass of CO2 to moles. The molar mass of CO2 is 44.01 g/mol (12.01 for C + 2*16.00 for O), so 0.22 g of CO2 is 0.22 g / 44.01 g/mol = 0.005 moles. The volume is given as 50 L (which is 0.05 m^3, since 1 m^3 = 1000 L), and the temperature is 305 K. The ideal gas constant R can be used in various units, but for this calculation, we'll use 8.314 (m^3·kPa)/(K·mol). Plugging the values into the ideal gas law equation gives:P = nRT/V = (0.005 moles * 8.314 kPa·m^3/(K·mol) * 305 K) / 0.05 m^3 = 25.4 kPaTherefore, the pressure exerted by the gas is closest to 25 kPa.

50 L Container at 305 K Holds a 0