A 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

677.7 mmHg

Explanation:

This is Dalton's law, where you add each partial pressure into total.

You are given total pressure of 692.2 mmHg

Partical pressure of water is: 14.5 mmHg

To find the partial pressure of O2, you subtract the total pressure and the given vapor pressure of water.

If you want the answer in atm, it would be: 0.892 atm

677.7 mmHg X (1 atm/760 mmHg) = 0.892 atm

Hope this helps!

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.