What was the volume of this gas at the fermentation temperature of 36.5celcius and 1atm pressure?
2006-09-16 18:19:38 · 4 answers · asked by Muhammad F 1 in Education & Reference ➔ Higher Education (University +)
u would use --- V1/T1=V2/T2 -- derived from PV=nRT
the first volume divied by the first temp is equal to the second volume divided by the second temp *** [[[moles, ideal gas constant and pressure are not needed because it stays constant]]]
********when doing these problems always convert temperatures to the kelvin scale when in celsius----degrees Celsius + 273 = Kelvin
********20.1 C + 273= 293.1 K--T1
********36.5 C + 273= 309.5 K--T2
V1/T1=V2/T2
(.78L)/(293.1 K) = V2/(309.5 K)
^^now solve for V2
V1 V2
----- = ----- ^^ since a porportion just cross-multiply and
T1 T2 divide
^^ you now have:
V1(T2)
----------- = V2 ^^Now substitute and slove for V2
T1
.78 L (309.5 K)
---------------------- = V2 ^^^Note: your temperature units will
293.1 K cancel here--> K / K = 1 the
same way you would simplify fractions
The answer is .82 L.
2006-09-16 18:55:03 · answer #1 · answered by ajm_jr_2005 2 · 2⤊ 0⤋
The first answer may be right, checking...
Yup, looks good. 0.82 L
From the ideal gas equation,
PV=nRT Where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is the absolute temperature in Kelvin.
You can setup a ratio of initial condition and final condition.
(P1V1)/(P2V2) = (n1R1T1)/(n2R2T2)
Where 1 is the initial condition, and 2 is the final condition.
The number of moles did not change, neither did the gas constant, or the pressure. So these cancle out from the top and bottom of each equation leaving.
(V1/V2)=(T1/T2)
You need to rearange the equation to solve for V2
V1*( T2/T1)=V2
20.1 C converted to Kelvin
K = C +273.15
K= 20.1 C +273.15 = 293.25 K
K2= 36.5C + 273.15 = 309.65 K
0.78L * ( 309.65 K / 293.25 K ) = 0.8236 L
Rounding to 2 significant digits, is 0.82 L
Austin Semiconductor
2006-09-16 19:41:55 · answer #2 · answered by Austin Semiconductor 5 · 1⤊ 0⤋
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2016-11-04 12:59:28 · answer #3 · answered by hultman 4 · 0⤊ 0⤋
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2016-11-27 19:46:05 · answer #4 · answered by Anonymous · 0⤊ 1⤋