Answer:
Correct option : "The mechanism results in a carbocation rearrangement in which a methyl shift occurs"
Explanation:
In the first step, 2,2-dimethyl-1-propanol gets protonated.
In the second step, a carbocationic intermediate is produced from removal of
.
In the third step, shifting of methyl group occurs to produce more stable carbocationic intermediate.
In the fourth step,
attacks the stable carbocation to produce 2-bromo-2-methylbutane.
So, correct option : "The mechanism results in a carbocation rearrangement in which a methyl shift occurs"
Full reaction mechanism has been shown below.
Answer:
![m=0.42m](https://tex.z-dn.net/?f=m%3D0.42m)
![Tb_{sol}=78.9^oC](https://tex.z-dn.net/?f=Tb_%7Bsol%7D%3D78.9%5EoC)
Explanation:
Hello,
In this case, we use the boiling point elevation colligative property equation for both ethanol and carbon tetrachloride as shown below:
![Tb_{sol}-Tb_{et}=Kb_{et}m\\Tb_{sol}-Tb_{CTC}=Kb_{CTC}m](https://tex.z-dn.net/?f=Tb_%7Bsol%7D-Tb_%7Bet%7D%3DKb_%7Bet%7Dm%5C%5CTb_%7Bsol%7D-Tb_%7BCTC%7D%3DKb_%7BCTC%7Dm)
Now, since both the boiling point and the concentration of the solutions are equal, we solve a 2x2 system of lineal equations:
![\left \{ {{Tb_{sol}-1.22m=78.4} \atop {Tb_{sol}-5.03m=76.8}} \right.](https://tex.z-dn.net/?f=%5Cleft%20%5C%7B%20%7B%7BTb_%7Bsol%7D-1.22m%3D78.4%7D%20%5Catop%20%7BTb_%7Bsol%7D-5.03m%3D76.8%7D%7D%20%5Cright.)
Subtracting the equations one obtains the molality (concentration):
![Tb_{sol}-Tb_{sol}-5.03m+1.22m=76.8-78.4\\-3.81m=-1.6\\m=0.42m](https://tex.z-dn.net/?f=Tb_%7Bsol%7D-Tb_%7Bsol%7D-5.03m%2B1.22m%3D76.8-78.4%5C%5C-3.81m%3D-1.6%5C%5Cm%3D0.42m)
Finally, solving for the boiling temperature of the solution one obtains:
![Tb_{sol}=Kb_{et}m+Tb_{et}\\Tb_{sol}=1.22^oC/m*0.42m+78.4^oC\\Tb_{sol}=78.9^oC](https://tex.z-dn.net/?f=Tb_%7Bsol%7D%3DKb_%7Bet%7Dm%2BTb_%7Bet%7D%5C%5CTb_%7Bsol%7D%3D1.22%5EoC%2Fm%2A0.42m%2B78.4%5EoC%5C%5CTb_%7Bsol%7D%3D78.9%5EoC)
Best regards.
Answer:- 88 kPa.
Solution:- The level of mercury in the atmospheric arm that is the open arm is 83 mm. It indicates the gas pressure is 83 mm higher than the atmospheric pressure.
gas pressure = height of mercury level in open tube in mm + atmospheric pressure
Let's convert this 83 mm pressure to kpa since the atmospheric pressure is given in kPa and the answer is also asked to report in kPa.
mmHg is converted to atm first and then atm is converted to kpa.
760 mmHg = 1 atm
and 1 atm = 101.325 kPa
![83mmHg(\frac{1atm}{760mmHg})(\frac{101.325kPa}{atm})](https://tex.z-dn.net/?f=83mmHg%28%5Cfrac%7B1atm%7D%7B760mmHg%7D%29%28%5Cfrac%7B101.325kPa%7D%7Batm%7D%29)
= 11 kPa
Atmospheric pressure is 76.9 kPa.
gas pressure = 11 kPa + 76.9 kPa
gas pressure = 87.9 kPa
If we think about sig figs rule then 87.9 should be round to 88 as in addition we go with least number of decimal places. 11 kPa does not have any decimal places and so the gas pressure is 88 kPa.
Answer:
False. The balance equation for the redox reaction is:
2Fe + 3CuSO₄ → 3Cu + Fe₂(SO₄)₃
Explanation:
Let's think the half reactions:
Fe → Fe³⁺ + 3e⁻
The Fe increase the oxidation state. This is the oxidation, where Fe changes from 0 to +3
Cu²⁺ + 2e⁻ → Cu
This is the reduction. Cu changes from 2+ to 0
We multiply the half reaction x2 and x3 to balance the electrons
2Fe → 2Fe³⁺ + 6e⁻
3Cu²⁺ + 3e⁻ → 3Cu
And we sum both
2Fe + 3Cu²⁺ + 6e⁻ → 3Cu + 2Fe³⁺ + 6e⁻
The electrons are cancelled, so the balance reaction is:
2Fe + 3CuSO₄ → 3Cu + Fe₂(SO₄)₃
Answer: C(s) + O2(g) --> CO2(g)12g (C) .... 50.8g (O2)................. initial amounts0g(C) .........18.8g(O2) ................. amounts when reaction completeThat means that C was the limiting reactant, and the amount of CO2 is based on the amount of carbon that burned. Covert 12 grams of carbon to moles. The moles of CO2 will be the same, since they are in a 1:1 mole ratio. Then convert the moles of CO2 to grams.12g C x (1 mol C / 12.0 g C) x (1 mol CO2 / 1 mol C) x (44.0g CO2 / 1 mol CO2) =44 g of CO2