SO2 molecular weight = 64. 576/64 = 9 so 576g = 9 moles.
1 mole of gas occupies 22.4 liters at STP.
So 9 x 22.4 = 201.6 liters.
The volume of 72 grams of SO2 is 27,4 L.
T = 35 degrees celsius = 308.15 degrees KelvinP = 97 atmV = ?n = 16.0 g SO2 / 64.06 g SO2 = 0.250 mol SO2
Divide mass of 128 g SO2 by its molar mass of 64.066 g.mol−1 SO2 and you get the number of moles: 1.9979 = 2.00 mole SO2
1 mole SO2 weights 32+2*16 = 64 gram S + 2*O and it's volume is 22.4 l You can do with that to calculate density (g/L) ?
The mass of sulfur is 50,04 g.
The volume of 72 grams of SO2 is 27,4 L.
Assuming standard temperature and pressure: 1 mole (64.1 g) of SO2 occupies 22.4 liters 72.0 g SO2 occupies (72.0/64.1) x 22.4 liters
1 mole of gas occupies 22.4 liters at STP. Therefore 3.5/22.4 = 0.15625 moles of SO2. There are thus 0.15625 moles of O2 needed to react with solid sulfur because S + O2 ---->SO2. 0.15625 moles of oxygen occupies 0.15625 x 22.4 liters = 3.5 liters O2 required.
T = 35 degrees celsius = 308.15 degrees KelvinP = 97 atmV = ?n = 16.0 g SO2 / 64.06 g SO2 = 0.250 mol SO2
1 mole SO2 = 64.064g SO2 0.45g SO2 x 1mol SO2/64.064g SO2 = 0.0070 mole SO2
.75 moles times 64 grams/mols = 48 grams
72 grams SO2 (1 mole SO2/64.07 grams)(6.022 X 1023/1 mole SO2) = 6.8 X 1023 molecules of sulfur dioxide ============================
48.045
25.6 g
5
volume is 3.85 cubic dm. or litre.....
.75