Final answer:
The mass of oxygen gas with a volume of 320 ml at 17°C and 2 atm pressure is calculated using the Ideal Gas Law (PV = nRT), with temperature in Kelvins, volume in liters, and the ideal gas constant. After determining the number of moles, the mass is found by multiplying by the molar mass of O2.
Step-by-step explanation:
To calculate the mass of oxygen gas whose volume is 320 ml at 17°C and 2 atm pressure, we can use the Ideal Gas Law equation, which is PV = nRT. In this formula:
• P represents the pressure of the gas
• V represents the volume of the gas
• n represents the number of moles of the gas
• R is the ideal gas constant
• T is the temperature in Kelvins
Before we substitute the values into the equation, we need to convert the given temperature to Kelvins by adding 273 to the Celsius temperature. So, T = 17 + 273 = 290 K. We also need to convert the volume to liters by dividing the ml value by 1000. Thus, V = 320 ml / 1000 = 0.320 L. The pressure is already given in atm, so we can use it directly.
The ideal gas constant R can be used as 0.0821 L·atm/mol·K. Now we can rearrange the Ideal Gas Law equation to solve for n (the number of moles): n = PV / RT. Substituting the values gives us n = (2 atm × 0.320 L) / (0.0821 L·atm/mol·K × 290 K). Calculating this, we find the number of moles of oxygen gas.
After finding the number of moles, we can calculate the mass of oxygen gas by using the molar mass of O2, which is approximately 32.00 g/mol. Therefore, the mass of the gas (m) can be calculated as m = n × molar mass. By multiplying the number of moles by the molar mass of oxygen, we get the mass of oxygen gas in grams.
It is important to note that these calculations are based on the assumption that the gas behaves ideally, which is a common approximation for gases at standard temperature and pressure conditions.