2007-03-08 18:07:02 · 4 answers · asked by Lightning 1 in Science & Mathematics ➔ Chemistry
Let's assume that this gas is ideal and at standard pressure and temperature (typically a good approximation, especially since the info is excluded in the question). One mole of any gas has a volume of 22.4 liters.
Also, recall that the molecular weight of N is 14 g/mole so that of N2 is 28.0 g/mole.
The volume of 46.0 g of N2 is:
46.0 g N2 x (1 mole N2 / 28.0 g N2) x (22.4 L N2 / 1 mole N2) = 36.8 L N2
2007-03-08 19:39:24 · answer #1 · answered by Sam 5 · 0⤊ 0⤋
28 grams of N2 gas = one mole of this gas, and at STP circumstances, it could have a quantity of twenty-two.4 liters. to establish that the N2 to occupy a quantity of 40 4.8 liters, you will would desire to decrease the strain on the gas in a million/2. so the respond would be, authentic if the strain is one a million/2 ecosystem and the temperature is 0 stages C or 273 stages ok
2016-12-18 09:03:04 · answer #2 · answered by ? 4 · 0⤊ 0⤋
46.0 g N2 x (1 mole N2 / 28.0 g N2) x (22.4 L N2 / 1 mole N2) = 36.8 L N2
at stp
2007-03-09 03:35:20 · answer #3 · answered by Cody B 2 · 0⤊ 0⤋
You need to know the pressure and temperature. The density of nitrogen gas is 1.251 g/L at 0ºC and 101.325 kPa, so the volume is 46/1.251 L under those conditions.
2007-03-08 18:16:19 · answer #4 · answered by gp4rts 7 · 0⤊ 0⤋