Chlorine is widely used to purify municipal water supplies and to treat swimming pool water. Suppose that the volume ?
Chlorine is widely used to purify municipal water supplies and to treat swimming pool water. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 895 torr and 25 ∘C.
How many grams of Cl2 are in the sample?
What volume will the Cl2 occupy at STP?
At what temperature will the volume be 14.50 L if the pressure is 873 torr?
At what pressure will the volume equal 5.50 L if the temperature is 58 ∘C?
- hcbiochemLv 71 month agoFavorite Answer
Use the ideal gas law: PV = n RT
Since all pressures are given in torr, use R = 62.37 L torr / mol K
895 torr (8.70 L) = n (62.37 L torr/molK) (298 K)
n = 0.419 mol Cl2
Mass Cl2 = 0.419 mol X 70.9 g/mol = 29.7 g Cl2
To calculate the volume of gas at STP, you can either calculate it using:P1V1/T1 = P2V2/T2 where P2 = 760 torr and T2= 273 K
Or, you can use the idea that at 1 atm pressure and 273 K, 1 mole of gas has a volume of 22.4 L. So,
0.419 mol X 22.4 L/mol = 9.38 L
P1V1/T1 = P2V2/T2
895 torr (8.70 L) / 298 K = 873 (14.50 L) / T2
T2 = 484 K = 211 C
Use this same formula to solve the last one.