Explanation:
The only flaw I can find is you squared 3 instead of cubing it and it will be 27X^4 instead of 9x^4.
This reduces the amount slightly, but the number is still incredibly high (about 10 ^ 5 L is what I've calculated). Your professor might want to point out that this will not be a effective experiment due to the large volume of saturated
The Ksp value of Ca(OH)2 on the site (I used 5.5E-6 [a far more soluble compound than Al(OH)3]) and estimated how much of it will be needed. My calculation was approximately 30 ml. If you were using that much in the experiment, it implies so our estimates for Al(OH)3 are right, that the high amount is unreasonably big and that Al(OH)3 will not be a suitable replacement unless the procedure was modified slightly.
Answer:
Incomplete precipitation of barium sulfate
Explanation:
The student has precipitated and digested the barium sulfate on his/her side. But on the addition of in the solution, the solution become cloudy. This happened because incomplete precipitation of barium sulfate by the student. When is added, there are still sulfate ions present in the solution with combines with and forms and the formation of this precipitate makes the solution cloudy.
Answer: The empirical formula is .
Explanation:
If percentage are given then we are taking total mass is 100 grams.
So, the mass of each element is equal to the percentage given.
Mass of C = 50.69 g
Mass of N= 19.71 g
Mass of H = 7.09 g
Mass of O = 22.51 g
Step 1 : convert given masses into moles.
Moles of C =
Moles of N=
Moles of H=
Moles of O =
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For C =
For N =
For H =
For O =
The ratio of C:N:H: O = 3:1:5:1
Hence the empirical formula is .
Answer:
<u>Option B is correct</u>
Explanation:
Step 1: Define volatility
In chemistry, the term volatility, is a way to describe how readily a substance transitions from a liquid phase to a gas phase, also called evaporating.
At a given temperature and pressure, a substance with high volatility is more likely to evaporate more quickly , while a substance with a lower volatility is more likely to be a liquid or solid, so not to evaporate or slower.
The higher the volatility, the higher the (vapor) pressure of a compound. Increasing temperature means the vapor pressure will also increase,
Step 2: In this case:
⇒ O<u>ption A is false</u> because the pressure will be higher when volatility is higher.
<u>⇒ Option B is correct</u> because higher volatility means evaporating more quickly
<u>⇒ Option C is false</u> because higher volatility means higher pressure. When pressure increases, the surface tension decreases.
<u>⇒ Option D is false</u> because when the volatility is higher, the liquid/gas escape the container, easier, so there will be less resistance.