1)a If a sample of oxygen gas has a volume of 4.89 L at 20.0 °C and a pressure of 1.20 atm. If the temperature was increased to 56.0 °C then what would its resultant volume be (in L?) Assume the new pressure is 1.20 atm.
b At STP, 297.0 mL of a certain gas has a mass of 0.366 g. What is a possible identity of this gas?
Select one:
a. O3
b. Cl2
c. C2H6
d. O2
e. N2
volume v1 = 4.89 l v2 = ?
temperature t1 = 20 c = 293k t2 = 56c = 329k
pressure p1 and p2 is 1.20 atm
no change in pressure so p1 = p2
then v1 / t1 = v2 / t2
v2 = v1*t2 / t1
v2 = 4.89 * 329 / 293
v2 = 5.49 litres
answer new volume is = 5.5 litres
no of moles at STP as follows
at STP 1 mole occupies 22.4 litres
1mole----------------------> 22.4 litres
? --------------------------> 0.297 litres
=>0.297/22.4 = 0.0132258 moles
answer is ( e ) = 0.366g / 0.0132258 moles = 27.6 g / mol i.e = 28 g / mol i.e N2
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