Yes M.

asked • 03/16/23

I need help on this chemistry problem, thank you!

A gas has a volume of 3.56 LL at 0 ∘C. What final temperature, in degrees Celsius, is needed to change the volume of the gas to each of the following, if n and P do not change?

10.4 L

Express your answer to three significant figures in degrees Celsius.



Sharon K.

tutor
525 degrees Celcius. According to Charles law, volume over temperature initial is how you set up the problem. So then you're going to have a final volume and temperature, V over T. Using cross multiplication you can solve for the final temperature which is five hundred and twenty five degrees celsius. Before I got this I had to convert celsius to kelvin but to keep it simple the answer is five hundred and twenty five degrees celsius
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03/23/23

1 Expert Answer

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J.R. S. answered • 03/27/23

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V1 = initial volume = 3.56 L

T1 = initial temperature in Kelvin = 0ºC + 273 = 273K

V2 = final volume = 10.4 L

T2 = final temperature in Kelvin = ?

Use V1/T1 = V2/T2 (constant pressure = Charles' Law)

3.56 L / 273k = 10.4 L / T2

T2 = 797.5 K

Converting to Celsius...

797.5 -273.15 = 524.38ºC

Rounding to 3 sig. figs. we get 524ºC

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