Final answer:
Using the Ideal Gas Law PV = nRT and the given conditions, the number of moles of the gas is calculated and multiplied by the molar mass to determine that approximately 3.25 grams of gas are present in the container.
Step-by-step explanation:
To determine how many grams of gas are present in the given conditions, we need to apply the Ideal Gas Law, which is 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. To calculate the number of moles (n), we rearrange the Ideal Gas Law to n = PV/(RT). The pressure (P) is 108 kPa (which is 108,000 Pa), the volume (V) is 1.8 liters (which needs to be converted to cubic meters by multiplying by 0.001 to get 0.0018 m³), and the temperature (T) is 26.7°C (which is 299.85 K when you add 273.15). The ideal gas constant (R) is 8.314 J/(mol·K). Plugging in these values gives us n = (108,000 Pa × 0.0018 m³) / (8.314 J/(mol·K) × 299.85 K), which equals about 0.0739 moles of gas. Once we have the number of moles, we use the molar mass of the gas, 44 g/mol, to find the mass of the gas by multiplying the number of moles by the molar mass (m = n × molar mass). Hence, 0.0739 moles × 44 g/mol gives us approximately 3.25 grams of the gas present in the container.