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Question

x C Mechanical Engineering x Secure l https://edugen wileyplus.com/edugen/nti/main uni Return to Blackboard PLUS Hein, Foundations of College Chemistry, Fourteenth Edition Help I (b) mass mass oh-L...................................... times mass of H2 exact number, no tolerance Your answer is partialy correct. Try again. (c) number of moles According to UAMogadroslaw J, equal volumes of H2 and o2 at the same Tand p have Hewer Incorrect. Are the gases at the same temperature? (d) average kinetic energy of the molecules average kinetic energy of O2 average kinteic energy of H2 Incorrect. Did you substitute the correct molar mass values into Graham's Law of effusion? moles.

Explanation / Answer

mass of one mole O2 = 32 g

mass of one mole H2 = 2 g

Mass of O2 is 32/2 = 16 times mass of H2 Answer 16 times

At same temperature and pressure same volume of H2 and O2 will contain equal no of O2 and H2

Answer equal to O2

Temperature measures the average kinetic energy of the molecules of a substance.

Answer equal

We know that O2, being heavier, will be the slower. So, let us assign it a rate of 1 and let it be r2. That way, its rate is in the denominator.

Now, we use Graham's Law, as the previous poster said:

x/1 = (32/2)

x = 4

So, hydrogen effuses 4 times as fast as oxygen. Or, oxygen effuses only 1/4 as fast as hydrogen.

weight of one mole of H2 = 2 g = 0.002 kg

Volume of one mole of H2 at STP = 22.4 L = 0.0224 m3

density of H2 = 0.002 kg / 0.0224 m3 = 0.0893 kg/m3

density of O2 = 32 g / 0.0224 m3 = 0.032 kg / 0.0224 m3 =1.4286 kg/m3

Density of O2 = 1.4286 / 0.0893 = 16 times density of H2

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