Rank the following gases in order of decreasing rate of effusion. Rank from the highest to lowest effusion rate. To rank items as equivalent, overlap them. F2 He C5H10 H2 PH3

To Rank from the highest to lowest effusion rate; we have;. H2 > He > PH3 > F2 > C5H10

From Graham's law of diffusion;

At constant temperature band pressure, the rate of diffusion of a gas is inversely proportional to the square root of its Molecular weight.

In essence, the heavier a gas, the slower is it's rate of diffusion or perhaps effusion as in this case.

The molecular weight of the gases given are as follows;

Therefore, since the lighter gases diffuses/effuses faster;

To Rank from the highest to lowest effusion rate; we have;

H2 > He > PH3 > F2 > C5H10

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H2, He, PH3, F2, C5H10

Explanation:

From Graham's law, we understood that lighter gas will diffuse faster than heavier gas under same condition. Graham's law of diffusion states as follow:

The rate (R) of diffusion of a gas is inversely proportional to the square root of its density (D) provided temperature and pressure remains constant. Mathematically, it is represented as:

R & 1/√D

Recall:

Molar Mass (M) = 2 x vapour density (D)

M = 2D

R & 1/√M

From the above, we can see that the rate is inversely proportional to the square root of the molar mass of substance. This implies that lighter gas will diffuse faster.

Now, to rank the above from the highest to rate rate of effusion, let us determine the molecular weight of each substance. This is illustrated below:

Molar Mass of F2 = 19 x 2 = 38g/mol

Molar Mass of He = 4g/mol

Molar Mass of C5H10 = (12X5) + (10X1) = 70g/mol

Molar Mass of H2 = 2x1 = 2g/mol

Molar Mass of PH3 = 31 + (3x1) = 34g/mol

Now, we can rank the substance beginning from the highest to the lowest rate of effusion as follow:

Substance >> Molar Mass >> Rank

H2 >>>>>>>>> 2g/mol >>>>>> 1

He >>>>>>>>> 4g/mol >>>>>> 2

PH3 >>>>>>>> 34g/mol >>>>> 3

F2 >>>>>>>>>> 38g/mol >>>> 4

C5H10 >>>>>> 70g/mol >>>> 5

c most likely

hop this let me know if it is wrong

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey