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torisob [31]
3 years ago
9

Calculate the freezing point (Kf = 1.86 °C/m) of a 2.1m aqueous solution of KCl.

Chemistry
1 answer:
Wittaler [7]3 years ago
7 0

Answer:

The freezing point of the solution is - 3.90 °C.

Explanation:

  • We can solve this problem using the relation:

<em>ΔTf = (Kf)(m),</em>

where, ΔTf is the depression in the freezing point.

Kf is the molal freezing point depression constant of water = - 1.86 °C/m,

m is the molality of the solution (m = 2.1 m).

<em>∴ ΔTf = (Kf)(m)</em> = (-1.86 °C/m)(2.1 m) =<em> - 3.90 °C.</em>

<em>∵ The freezing point if water is 0.0 °C and it is depressed by - 3.90 °C.</em>

<em>∴ The freezing point of the solution is - 3.90 °C.</em>

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3 years ago
What volume of so2 is produced at 325 k and 1.35 atm when 15.0 grams of hcl reacts with excess k2so3?
vova2212 [387]
The volume of SO2 produced at 325k   is calculated as  below

calculate  the moles of SO2 produced  which  is calculated as follows

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by  use of mole ratio between  HCl to  SO2  which is  2:1 the moles of SO2 is therefore = 0.411 /2 =0.206  moles  of SO2

use the idea  gas  equation  to calculate the volume SO2
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