Question

You have 1.366 x 102 mL of oxygen gas (O2) at 7.55 x 102 mm of Hg and 70 oC.
What is the mass of the sample in milligrams?

Answer 1

Isn't this a case of PV=nRT?

Answer 2

Yes

Answer 3

Then just plug in and solve for n

Answer 4

I forget the unit requirements. Are the units right or does something have to be converted?

Answer 5

I think it's alright in this case. Is the answer 386.89?

Answer 6

Did you convert the temp to degrees Kelvin?

Answer 7

No. Hold on

Answer 8

770.1?

Answer 9

I forget what the ideal gas constant is.

Answer 10

I'm not sure either.

Answer 11

Well then how did you solve it?

Answer 12

It's not right.

Answer 13

I only have 30 minutes left to answer 10 questions, I'd appreciate rapid help!

Answer 14

What you are taking a timed test?

Answer 15

It's not a test, just an online assignment and the turn in time cuts off in 30 minutes so I'm pretty pressured right now.

Answer 16

62.36367=R if volume is in L, temp in degrees Kelvin and pressure in mm of Hg

Answer 17

Is R the mass?

Answer 18

R is the ideal gas constant

Answer 19

n is the number of moles.

Answer 20

The question was dismissed because I accidently reset it.

Now:
You have 4.108 x 102 mL of oxygen gas (O2) at 7.19 x 102 mm of Hg and 23 oC.
What is the mass of the sample in milligrams?

Answer 21

That is exactly the same problem with different numbers.

Answer 22

I still don't know how to set it up! Do this one for me so I can follow the steps please?

Answer 23

Change the mL to liters

Answer 24

If a gas has a volume of 7.1 L at a temp of 22 Degrees Celsius and a pressure of 3.1 atm, how many moles of gas are present?

Answer 25

R=82.05736
Now since you have changed the units the constant has changed.
And you have to change the L to ml

Answer 26

7.1L= 7100 mL
22 degrees Celsius = 295 degrees Kelvin
so:
\[3.1(7100)=n(82.05736)(295)\]

Answer 27

Solve for n