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

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

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.