sample of oxygen is collected over water at a total pressure of 692.2 mmHg at 17°C. The vapor pressure of water at 17°C is 14.5 mmHg. The partial pressure of the O2

677mmHg

Explanation:

In answering this question, we use Dalton's law of partial pressures which states that in a mixture of two or more non-reacting gases, the total pressure  is equal to the sum of the partial pressures of the individual gases making up the mixture.

From the question, the gases are oxygen and water vapour.

Therefore the total pressure () is the sum of the partial pressure of oxygen () and the partial pressure of water vapour ()

= +     -----------------(i)

= 692.2mmHg

= 14.5mmHg

Substitute these values into equation (i) as follows;

692.2 = + 14.5

= 692.2 - 14.5

= 677.7

Therefore, the partial pressure of oxygen is 677mmHg

Because electrons have negligible mass, to account for the mass of the isotope, there must be 16 neutrons, 16 neutrally charged, massive, fundamental particles present in the sulfur nucleus. and thus finally, if we have the 32s2− ion, there are 18 electrons, 16 protons, and 16 neutrons.

Idon’t know what the answer is i wish i could