How many molecules are there in 4.00 L of oxygen gas at 500 C and 50.0 Torr

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I would appreciate it if someone could check and correct my work. Here’s the question: How many molecules are present in 4.00 L of oxygen gas at a temperature of 500 °C and a pressure of 50.0 Torr? 
Using the ideal gas law, PV = nRT, I converted the pressure: 50.0 Torr = 0.066 atm, and the temperature: 500 °C = 773 K. The ideal gas constant R is 0.0821 L·atm/(K·mol). 
Applying these values in the equation, we have: 
(0.066 atm) × (4.00 L) = n × (0.0821 L·atm/(K·mol)) × (773 K).
From this, I calculated the number of moles (n) and then converted moles to molecules using Avogadro's number (6.02 × 10^23). 
My final result is approximately 2.51 × 10^21 molecules.

Anonymous · Accepted Answer

(Pressure in atmospheres) * (Volume in liters) = (number of moles) * (Ideal gas constant) * (Temperature in ˚K)
 1 atm = 760 torr, P = 50/760 atm
V = 4.00 L
Ideal gas constant = 0.0821
T = 500 + 273 = 773˚K
50/760 * 4.00 = n * 0.0821 * 773
n = (50/760 * 4.00) ÷ (0.0821 * 773) 
This is the number of moles of oxygen in the container.
1 mole = 6.02 * 10^23 molecules
Number of molecules = 6.02 * 10^23 * Number of moles
Number of molecules = 6.02 * 10^23 * (50/760 * 4.00) ÷ (0.0821 * 773)
Number of molecules ≈ 2.496 * 10^21 
Rounded to 3 significant digits, the answer is 2.50 * 10^21 molecules.
This is the number of molecules of oxygen in the container.
I suggest that you do not round your answers as you calculate.

Anonymous · Answer

ans. is correct!

Anonymous

How many molecules are there in 4.00 L of oxygen gas at 500 C and 50.0 Torr

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