Answer:
(3R,4R)-4-bromohexan-3-ol
Explanation:
In this case, we have reaction called <u>halohydrin formation</u>. This is a <u>markovnikov reaction</u> with <u>anti configuration</u>. Therefore the halogen in this case "Br" and the "OH" must have <u>different configurations</u>. Additionally, in this molecule both carbons have the <u>same substitution</u>, so the "OH" can go in any carbon.
Finally, in the product we will have <u>chiral carbons</u>, so we have to find the absolute configuration for each carbon. On carbon 3 we will have an "R" configuration on carbon 4 we will have also an "R" configuration. (See figure 1)
I hope it helps!
Igneous <span>rock ! Of course oh how i miss middle school.........</span>
Answer:
7. genetics because hereditary is not the study of hereditary.
8. is hereditary because it is the study of how things pass on to next generation what is inherited.
Answer:
The mass of tin is 164 grams
Explanation:
Step 1: Data given
Specific heat heat of tin = 0.222 J/g°C
The initial temeprature of tin = 80.0 °C
Mass of water = 100.0 grams
The specific heat of water = 4.184 J/g°C
Initial temperature = 30.0 °C
The final temperature = 34.0 °C
Step 2: Calculate the mass of tin
Heat lost = heat gained
Qlost = -Qgained
Qtin = -Qwater
Q = m*c*ΔT
m(tin)*c(tin)*ΔT(tin) = -m(water)*c(water)*ΔT(water)
⇒with m(tin) = the mass of tin = TO BE DETERMINED
⇒with c(tin) = the specific heat of tin = 0.222J/g°C
⇒with ΔT(tin) = the change of temperature of tin = T2 - T1 = 34.0°C - 80.0°C = -46.0°C
⇒with m(water) = the mass of water = 100.0 grams
⇒with c(water) = the specific heat of water = 4.184 J/g°C
⇒with ΔT(water) = the change of temperature of water = T2 - T1 = 34.0° C - 30.0 °C = 4.0 °C
m(tin) * 0.222 J/g°C * -46.0 °C = -100.0g* 4.184 J/g°C * 4.0 °C
m(tin) = 163.9 grams ≈ 164 grams
The mass of tin is 164 grams
Answer:
Explanation:
From the information given :
we can understand the solute is glucose and the solvent is water,
So, the weight of glucose = 20.23 g
the molecular weight of glucose = 180.2 g/mol
weight of water = 95. 75 g
the molecular weight of water = 18.02 g/mol
pure vapor pressure of water 
at 27°C
moles of glucose = weight of glucose/ molecular weight of glucose
= 20.23/180.2
= 0.11 mole
moles of water = weight of water / molecular weight of water
= 95.75/18.02
= 5.31 mole
mole fraction of glucose 
(moles of glucose)/(moles of glucose+ moles of water)
0.11/(0.11 + 5.31)
0.0203
mole fraction of glucose 
(moles of water)/(moles of water+ moles of glucose)
5.31/ (5.31 + 0.11)
0.9797
Using Raoult's Law:
where:
= vapor pressure of the solution
= total vapor pressure of the solution
= vapor pressure of the solvent in the pure state
= mole fraction of solvent i.e. water
95.75 × 0.9797
93.81 mmHg
the total vapor pressure of the solution = 93.81 mmHg
