Asked by Kevin
An ideal gas with an initial volume of 96L, temperature of 277K, and 7.3mol is permitted to come to a second state with a volume of 450mL and a temperature of 203C. Show the calculation for the final number of moles of gas in the system.
(P1)(V1)/(n1)(T1)=(P2)(V2)/(n2)(T2)
(P1)(96L)/(7.3mol)(277K)=(P2)(.45L)/(x)(476K)
Does it matter if you aren't given pressure? Can you just throw a 1 in there or do you need to use PV=nRT to solve? If not, I got 9.478mol. Is that right?
(P1)(V1)/(n1)(T1)=(P2)(V2)/(n2)(T2)
(P1)(96L)/(7.3mol)(277K)=(P2)(.45L)/(x)(476K)
Does it matter if you aren't given pressure? Can you just throw a 1 in there or do you need to use PV=nRT to solve? If not, I got 9.478mol. Is that right?
Answers
Answered by
Olereb48
Assume pressure is constant. It will cancel out of the combined law expression.
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