Complete Question
Question 096 Propose a three-step synthetic sequence to accomplish the transformation below.
Option 1 => 1) HBr, ROOR; 2) t-BuOK; 3) CH3CH2CCNa
Option 2 => 1) NaOEt; 2) HBr, ROOR; 3) CH3CH2CCNa
Option 3 => 1) t-BuOK; 2) NaNH2; 3) CH3CH2CCNa
Option 4 => 1) CH3CH2CH2CH2Br; 2) NaOEt; 3) HBr, ROOR
Option 5 => 1) t-BuOK; 2) HBr, ROOR; 3) CH3CH2CCNa
Option 6 => 1) NaOEt; 2) NBS, hν; 3) NaSBu
Answer:
The correct option is option 5
Explanation:
The mechanism of the reaction is shown on the first uploaded image
Best Answer
1 mole of a substance contains 6.022x10^23 "units" of that substance.
So 0.187 mol of Na+ is 1.13x10^23 ions (6.022x10^23 x 0.187).
Answer:
The partial pressure of Ar is 356.04 mm Hg (= 0.4685 atm)
Explanation:
<u>Step 1:</u> Data given
A mixture of three gases has a total pressure of 1380 mm Hg (=1.81579 atm) at 298 K
Moles of CO2 = 1.27 moles
Moles of CO = 3.04 moles
Moles of Ar = 1.50 moles
<u>Step 2:</u> Calculate total number of moles
Total number of moles = n(CO2)+ n(CO)+ n(Ar) = 1.27 mol+ 3.04 mol+ 1.50 mol = 5.81 moles
<u>Step 3:</u> Calculate mol fraction Ar
Mol fraction Ar = 1.50 mol/5.81 mol = 0.258
<u>Step 4</u>: Calculate partial pressure
1380 mm Hg * 0.258 moles Ar = 356.04 mm Hg = 0.4685 atm
The partial pressure of Ar is 356.04 mm Hg (= 0.4685 atm)
Answer:
C
Explanation:
no. of moles = no. of atoms/ Avogadro's number
0.5= N/6.02×10^23
N= 3.01×10^23
