A gas sample with a constant number of gas molecules and at a constant temperature has a volume of 5.0 L at 50 mmHg pressure. The volume of the container can be varied. What would the gas sample volume be (in Liters) if the pressure of the gas increased to 500 mmHg?

.5 L

Explanation:

- Start with the Ideal Gas Law. This equation will be P1V1T2=P2V2T1

- Next, take out temperature because that is not given and therefore constant.

- Rearrange the equation. You should get V2=V1P1/P2

- Fill in with variables. You should get V2=((5.)(50))/500

- Solve and you will get .5L

- Lastly, you can check this by knowing that P and V at constant T have an inverse relationship. Hence, volume went down, while pressure went up.

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.