A sample of gas occupies 5mL at STP. At what pressure would this sample occupy 500 mL if the temperature is changed to 525° C? Answer in units of torr.
I tryed something like 4 times but it's always wrong, i don't know why!
I tryed something like 4 times but it's always wrong, i don't know why!
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You can also use the combined gas law: P1V1/T1 = P2V2/T2. This keeps you from having to know the number of moles of gas. But temperature must be in Kelvin not Celcius.
(760 Torr x 5 mL) / 273 K = (P2 x 500 mL) / 798
P2 = (760 Torr x 5 mL x 798 K) / (273 K x 500 mL)
P2 = 22.2 Torr
(760 Torr x 5 mL) / 273 K = (P2 x 500 mL) / 798
P2 = (760 Torr x 5 mL x 798 K) / (273 K x 500 mL)
P2 = 22.2 Torr
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PV=nRT you can figure out n because you know everything with the first statement
then use PV=nRT again to figure out P, MAKE SURE YOU ARE USING KELVINS NOT CELSIUS!
then use PV=nRT again to figure out P, MAKE SURE YOU ARE USING KELVINS NOT CELSIUS!