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

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If someone would check and or correct my work that would be appreciated.Q: How many molecules are there in 4.00 L of oxygen gas at 500 C and 50.0 TorrPV=nRT50 torr = .066 atm500 C = 773 K And the constant would be .08210.066 x 4 = moles x 0.082 x 773therefore there are 0.004 moles x 6.02 x 10^23So there are 2.51 x 10^21 molecules

Prof. Carmelo Hilpert · Accepted Answer

(Pressure in atmospheres) * (Volume in liters) = (number of moles) * (Ideal gas constant) * (Temperature in ˚K) 1 atm = 760 torr, P = 50/760 atmV = 4.00 LIdeal gas constant = 0.0821T = 500 + 273 = 773˚K50/760 * 4.00 = n * 0.0821 * 773n = (50/760 * 4.00) ÷ (0.0821 * 773) This is the number of moles of oxygen in the container.1 mole = 6.02 * 10^23 moleculesNumber of molecules = 6.02 * 10^23 * Number of molesNumber 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.

Prof. Carmelo Hilpert · Answer

ans. is correct!

Jace Toy DDS

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

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