Question

A student collects 530 mL of CO gas at a pressure of 1.2 atm and a temperature of 17ºC. What is the volume of the gas at 0ºC and 1 atm?
(530 mL) x (1.2 / 1.0) x (273 / (17 + 273)) = 599 mL
@Frostbite is this right?

Answer 1

yes please

Answer 2

how does it look @Frostbite?

Answer 3

Please try calculate the number again.

Answer 4

(530 mL) x (1.2 / 1.0) x (273 / (17 + 273))
is this part right?

Answer 5

Yea it looks right, but can you try see what it gives again?

Answer 6

ok

Answer 7

598.717

Answer 8

what about sig digits?

Answer 9

wouldn't it be 590?

Answer 10

wait a sec... switch the temperature fraction.

Answer 11

i am so srry but I have to go grab dinner but I will be back in about 45 min.
will u still be here?

Answer 12

or will you be here tmrw?

Answer 13

lol ur like my fave tutor :)

Answer 14

yes my final answer is volume=676 is this right @Frostbite

Answer 15

You're given all the information, I don't know why you didn't just use the ideal gas law formula: \(PV = nRT\) to find moles. Then,
Rearrange to solve for volume, therefore you have: \(V = \LARGE \frac{nRT}{P}\)

Answer 16

:(

Answer 17

wait so how do I use the PV=nRT formula?

Answer 18

Did you change your temp to kelvin?

Answer 19

I actually dont know i dont have a calculator with me so maybe ur right or wrong.

Answer 20

yea

Answer 21

ok :)

Answer 22

thanks anyway!

Answer 23

Sorry I said something stupid. I made a wrong arrangement between the gas laws.

Answer 24

I'm so sorry, first now I see I did a fatal mistake:
We don't actually need \(n\), as it turns out it just go away:
\[\Large pV=nRT \to 1=\frac{ pV }{ nRT }\]
\[\Large \frac{ P _{1}V _{1} }{ nR T_{1} }=\frac{ P _{2}V _{2_{?}} }{ nRT _{2} }\]
The gas constant \(R\) and amount of substance \(n\) remain constant so:
\[\Large \frac{ P _{1}V _{1} }{ T _{1} }=\frac{ P _{2}V _{2} }{ T _{2} }\]
Ones again sorry, and thanks @abb0t you made me see it.

Answer 25

I never said your method was incorrect. I wa just suggesting another :P

Answer 26

Well it was incorrect :P