Answer: It tells you if your hyposthesis was incorrect or correct from the data. The data supports this because you tested and got your results correctly which will help you to form a hypothesis.
Explanation:
Answer is in a ph
oto. I can't attach it here, but I uploaded it to a file hosting. link below! Good Luck!
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Answer:
The rate of reaction changes by a factor 6.
Explanation:
Given the reaction is first order.
Let us assume the initial concentration of 
is 
and the initial concentration of 
is 
.
So, we can write the rate of the reaction as
![R=k[A][B]](https://tex.z-dn.net/?f=R%3Dk%5BA%5D%5BB%5D)
Where,
is the rate of reaction. And 
is the rate constant.
Also, the initial concentration of has been increased by 
, and the initial concentration of was increased by factor 
.
So, we have
![R'=k[1.5A][4B]\\R'=6k[A][B]\\R'=6R](https://tex.z-dn.net/?f=R%27%3Dk%5B1.5A%5D%5B4B%5D%5C%5CR%27%3D6k%5BA%5D%5BB%5D%5C%5CR%27%3D6R)
We can see the rate of reaction changes by a factor 6.
The freezing point depression is a colligative property which means that it is proportional to the number of particles dissolved.
The number of particles dissolved depends on the dissociation constant of the solutes, when theyt are ionic substances.
If you have equal concentrations of two solutions on of which is of a ionic compound and the other not, then the ionic soluton will contain more particles (ions) and so its freezing point will decrease more (will be lower at end).
In this way you can compare the freezing points of solutions of KCl, Ch3OH, Ba(OH)2, and CH3COOH, which have the same concentration.
As I explained the solution that produces more ions will exhibit the greates depression of the freezing point, leading to the lowest freezing point.
In this case, Ba(OH)2 will produce 3 iones, while KCl will produce 2, CH3OH will not dissociate into ions, and CH3COOH will have a low dissociation constant.
Answer: Then, you can predict that Ba(OH)2 solution has the lowest freezing point.
Answer:
Explanation:
Percent yield is the ratio of the amount actually produced to how much could theoretically be produced. It is found using this formula:
For this reaction, the theoretical or expected yield is 325.0 grams. The actual yield is 123.8 grams.
Divide.
Round to the nearest hundredth. The 9 in the hundredth place tells us to round the 0 to a 1 .
The percent yield is about <u>38.1%</u>
