Final answer:
To find the amount of argon gas that can fit in a 225-L container at a pressure of 112 kPa and a temperature of -10°C, we can use the ideal gas law equation. After calculating the number of moles of argon, we can multiply it by the molar mass to find the mass in grams. The correct answer is d) 402 g.
Step-by-step explanation:
To find the amount of argon gas that can fit in the 225-L container, we can use the ideal gas law equation: PV = nRT. Where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in kelvin. We need to convert the temperature from Celsius to kelvin by adding 273.15. Rearranging the equation to solve for the number of moles gives us n = PV / RT. Plugging in the values, we get n = (112 kPa)(225 L) / (8.314 kPa L/mol K)((-10°C + 273.15) K). Calculating this gives us approximately 16.8 moles of argon gas. The molar mass of argon is 39.95 g/mol, so to find the mass of argon in grams, we multiply the number of moles by the molar mass: 16.8 moles * 39.95 g/mol ≈ 670.56 g. Therefore, the correct answer is d) 402 g.