Two flasks of equal volume and at the same temperature contain different gases.

Question

Two flasks of equal volume and at the same temperature contain different gases. One flask contains 5.0 g of O2, and the other flask contains 5.0 g of H2. Is each of the following statements true or false? Explain.

a) True. Because the gases have the same volumes, they must have the same number of molecules.

b) False. Because the molar mass of O2 is greater than the molar mass of H2, 5.0g of O2 will contain fewer molecules than 5.0 g of H2.

c)False. Depending on the pressure each flask may contain different numbers of molecules.

Explanation / Answer

First statement is true but second ststement i.e. One flask contains 5.0 g of O2, and the other flask contains 5.0 g of H2. is false. It should be One flask contains 32.0 g of O2, and the other flask contains 2.0 g of H2. According to

One mole of an ideal gas will occupy a volume of 22.4 liters at STP (Standard Temperature and Pressure, 0

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