Answer:
We may utilise the ideal gas law to answer this problem, which links a gas's pressure, volume, number of moles, and temperature:
PV = nRT
where P denotes atmospheric pressure (atm), V denotes volume in litres (L), n is the number of moles, R denotes the gas constant (0.08206 Latm/(molK)), and T denotes temperature in Kelvin (K).
To begin, we must convert pressure from mmHg to atm and temperature from Celsius to Kelvin:
720 mmHg equals 0.947 atm
21°C = 294 K
Then, using the supplied parameters, we can solve for the volume using the ideal gas law:
V = nRT/P
(2.0 mol)(0.08206 Latm/(molK))(294 K)/(0.947 atm)
V ≈ 50.3 L
SOO the answer is , 2.0 moles of oxygen will occupy approximately 50.3 liters of volume at 720 mmHg and 21°C.
(im so sorry if its wrong)