Cuál es la densidad (g/ml) de un liquido de batería de automóvil, si tiene un volumen de 0,125 L y una masa de 155g¿?
1 answer:
You might be interested in
Answer : The final molarity of iodide anion in the solution is 0.0508 M.
Explanation :
First we have to calculate the moles of and
.
Molar mass of KI = 166 g/mole
and,
Now we have to calculate the limiting and excess reagent.
The given chemical reaction is:
From the balanced reaction we conclude that
As, 1 mole of KI react with 1 mole of
So, 0.0178 mole of KI react with 0.0178 mole of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and KI is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of
From the reaction, we conclude that
As, 1 mole of react to give 1 mole of
So, 0.0178 moles of react to give 0.0178 moles of
Thus,
Moles of AgI = Moles of anion = Moles of
cation = 0.0178 moles
Now we have to calculate the molarity of iodide anion in the solution.
Therefore, the final molarity of iodide anion in the solution is 0.0508 M.
Answer : Carbon tetrachloride, will show the greatest freezing point lowering.
Explanation :
For non-electrolyte solution, the formula used for lowering in freezing point is,
where,
= lowering in freezing point
= molal depression constant
m = molality
As per question, the molality is same for all the non-electrolyte solution. So, the lowering in freezing point is depend on the only.
That means the higher the value of , the higher will be the freezing point lowering.
From the given non-electrolyte solutions, the value of of carbon tetrachloride is higher than the other solutions.
Therefore, Carbon tetrachloride, will show the greatest freezing point lowering.