Answer:
1. This reaction is <u>(A) Exothermic .</u>
2. When the temperature is decreased the equilibrium constant, K: <u>(A) Increases</u>
3.When the temperature is decreased the equilibrium concentration of Co2:<u> (A) Increases</u>
Explanation:
1. The pink color predominates at low temperatures, indicating that the commodity is preferred.
This is a reaction that is <u>exothermic.</u>
2. As the decrease in the temperature , the equilibrium constant , K ;
equilibrium constant = 
=![\frac{[CO^2^+][Cl^-^4]}{CoCl^2^-_4}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BCO%5E2%5E%2B%5D%5BCl%5E-%5E4%5D%7D%7BCoCl%5E2%5E-_4%7D)
As the temperature drops, the concentration of
and 
rises, and K rises as well , thus it <u>increases </u>.
3. The equilibrium concentration of decreases as the temperature decreases:
When the temperature is lowered, the equilibrium shifts to the right , that is it <u>increases.</u>
Answer : The boiling point of the resulting solution is, 
Explanation :
Formula used for Elevation in boiling point :
or,
where,
= boiling point of solution = ?
= boiling point of water = 
= boiling point constant = 
m = molality
i = Van't Hoff factor = 1 (for non-electrolyte)
= mass of solute (sucrose) = 5.0 g
= mass of solvent (water) = 10.0 g
= molar mass of solute (sucrose) = 342.3 g/mol
Now put all the given values in the above formula, we get:
Therefore, the boiling point of the resulting solution is,
Answer:
Explanation:
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Answer: The molality of solution is 17.6 mole/kg
Explanation:
Molality of a solution is defined as the number of moles of solute dissolved per kg of the solvent.
where,
n = moles of solute
= weight of solvent in kg
moles of acetone (solute) = 0.241
moles of water (solvent )= (1-0.241) = 0.759
mass of water (solvent )= 
Now put all the given values in the formula of molality, we get
Therefore, the molality of solution is 17.6 mole/kg
