a) Calculate the mass in g of the compound Cs2S in 89 g of a 17.0% solution.
b) A 0.553 m3 of a gas originally at 125 oC must be reduced to a volume of 0.435 m3 at constant pressure. To what Celsius temperature must the sample be adjusted?
c) The reaction
2 Sb + 3 Cl2= 2 SbCl3
has a 62.3% yield. If 436 g of SbCl3 is obtained, what mass in g of Cl2 reacted?
thx...
2007-03-09 17:56:38 · 1 answers · asked by godrics 2 in Science & Mathematics ➔ Chemistry
a)
In 89 g of 17% solution,
mass of Cs2S = 89 x 0.17 = 15.13g
b)
Using V1/T1 = V2/T2 (constant pressure)
V1 = 0.553 m3
T1 = 125 + 273 = 398 K
V2 = 0.435 m3
(0.553)/(398) = (0.435)/T2
Temperature, T2 = 313 K = 40 oC
c)
3Cl2 to produce 2SbCl3
Yield = 62.3%
SbCl3 / Cl2 = 2/3 x 62.3/100
436 / Cl2 = 2/3 x 0.623
Cl2 = 1049.76g
2007-03-09 18:59:17 · answer #1 · answered by seah 7 · 1⤊ 0⤋