Answer:
To determine the volume of oxygen in liters at a pressure of 1.00 atm, we need to use the ideal gas law, which states that the volume of a gas is directly proportional to the pressure and temperature of the gas, and inversely proportional to the number of moles of gas present.
The ideal gas law can be written as:
PV = nRT
where P is the pressure of the gas (in atm), V is the volume of the gas (in liters), n is the number of moles of gas present, R is the gas constant (8.3145 J/mol·K), and T is the temperature of the gas (in K).
Since we are given that the pressure is 1.00 atm and the volume is 3.60 liters, we can rearrange the equation to solve for the number of moles of oxygen present:
n = PV / RT
Substituting the values given, we get:
n = (1.00 atm) x (3.60 liters) / (8.3145 J/mol·K) x T
Since the temperature is not given, we will assume that it is room temperature (approximately 293 K). Substituting this value, we get:
n = (1.00 atm) x (3.60 liters) / (8.3145 J/mol·K) x 293
Simplifying and calculating the value, we get:
n = 0.455 mol
Since we know the number of moles of oxygen present, we can now use the ideal gas law to calculate the volume of the gas:
V = nRT / P
Substituting the values given, we get:
V = (0.455 mol) x (8.3145 J/mol·K) x 293 / (1.00 atm)
Simplifying and calculating the value, we get:
V = 3.60 liters
Therefore, the volume of oxygen in liters at a pressure of 1.00 atm is 3.60 liters.
Step-by-step explanation: