Dont understand Charles' Law, but dont understand even more using the Ideal Gas Law to get to Charles's Law?

Question

For the following question use Charles's law, assuming that pressure and the number of moles of gas to be are constant.

1. V1 1.08L T1 25.4 C V2 1.33L T2?

2. V1 232 L T1 18.5 C V2 ? T2 96.2 C

Please Help!!!!

Answer 1

Charles Law: Vol and temp are directly proportional; so set up a proportion. Remember to change temperature to Kelvin by adding 273 to the celcius temp.

V1/T1 = V2/T2

in your q.1, T2 is your unknown; solve for it. The answer will be in Kelvin; if you need celcius, subtract 273.

in your q. 2 V2 is your unknown; solve for it.

To get Charles Law from Ideal Gas Law (PV = nRT) consider the following:

P1V1 = n1RT1: rearrange the T1 and P1 to get: V1/T1 = (n1R/P1)

then

P2V2 = n2RT2; rearrange the T2 and P2 to get: V2/T2 = (n2R/P1)

but in Charles Law n1=n2 and P1 = P2 (number of moles and pressure are consant; R is a constant) so you can write:

V1/T1 = (nR/P) = V2/T2 and so V1/T1 = V2/T2

(if a = b = c, then a=c)

Answer 2

just use V1 / T1 = V2 / T2

so 1.08 / (25.4 + 273) = 1.33 / T2
(you add 273 to temp so that it is in Kelvins)

232 / (18.5 + 273) = V2 / (96.2 + 273)

solve for the variables

Answer 3

for 2 instruments of circumstances, for substitute of temp only, use charles's with temps in Kelvin for 2 instruments of circumstances, for substitute of stress only, use boyle's, instruments do no longer remember as long as they are the two the comparable For one set of circumstances (e.g. no longer 2 temps or 2 pressures), the proper gasoline regulation is used . you additionally can %. those out because of the fact they might have grams or moles interior the situation. it could additionally be used for density problems with g/mL which you exchange to moles/L so instruments cancel.