Increasing the temperature of a reaction system that is exothermic and at 14. He
ID: 956170 • Letter: I
Question
Increasing the temperature of a reaction system that is exothermic and at 14. Henry's Law predicts that the solubility of a gas in a liquid increases with its partial pressure. 15. The value of Keq for the reaction between water vapor and dichlorine monoxide, H20(g) t c. will shift the position of chemical equilibrium towards equilibrium Explain Henry's Law in relation to Le Châtelier's Principle. Cl20 (g) 2HOCI(g) is 0.0900 at 25 °C. Determine the equilibrium concentrations of all three compounds if the starting concentrations of both reactants are 0.00432 M and no HOCl is present. 16. Two cubic containers (seen in the figure below) contain the same quantity of gas at the same temperature. Which cube contains gas with more entropy? If the sample on the right below is left unchanged, but the sample on the left below is cooled so that it condenses, which sample has the higher entropy? 1PT 17. Identify the processes as spontaneous or nonspontaneous 1 nhntevoltaic cell in a solar panel producing electricityExplanation / Answer
Data.
Keq = 0.0900
T = 25°C
Initial concentrations:
[Cl2O] = [H2O] = 0.00432 M
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Balanced equation
Cl2O + H2O <==> 2 HCLO
0.00432 0.00432 -
-x -x (+2x)
Eq (M).
(0.00432-x) (0.00432-x) 2x
The equilibrium constant is as follows;
Keq = [HClO]2 /[Cl2O][H2O]
by replacing the values you got:
0.0900 = 2x2 / (0.00432-x) (0.00432-x)
Square root of both sides of the equation to get,
0.3 = 2x / (0.00432 - x)
(0.00432 - x) 0.3 = 2x
From this clear: 0.00432 * 0.3 = 0.001296
0.001296 = 2x + 0.3x
0.001296 = 2.3x
x = 0.001296/2.3 = 0.000563 M
x = 5.63 x 10-4 M
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Concentrations on equilibrium are: (answers)
[HClO] = (2 x 5.63 x 10-4 M) = 1.126 x 10-3 M
[Cl2O] = (0.00432 M - 5.63 x 10-4 M) = 3.75 x 10-3 M
[H2O] = (0.00432 M - 5.63 x 10-4 M) = 3.75 x 10-3 M
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It's convenient to verify these answers calculating Keq with these equilibrium concentrations:
Keq = (1.126 x 10-3 M)2 / (3.75 x 10-3 M)2 = 0.09016
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Cheers!