Yes M.
asked • 03/16/23I 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.
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1 Expert Answer
J.R. S. answered • 03/27/23
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Ph.D. University Professor with 10+ years Tutoring Experience
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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Sharon K.
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 celsius03/23/23