the reagents necessary to convert alcohol to ketone
which involves oxidation of alcohols.
<h3>
What is oxidation of alcohols?</h3>
- Alcohol oxidation is a significant organic chemistry process. Secondary alcohols can be oxidized to produce ketones, while primary alcohols can be oxidized to produce aldehydes and carboxylic acids.
- In contrast, tertiary alcohols cannot be oxidized without the C-C bonds in the molecule being broken.
- In order to cause primary alcohols to oxidize into aldehydes
(dichromate)
/pyridine (Collins reagent)- Chromium pyridinium compound (PCC)
- Dichromate of pyridinium (PDC, Cornforth reagent)
- Periodinane by Dess-Martin
- Oxalyl chloride with dimethylsulfoxide (DMSO) for Swern
- oxidation of secondary alcohols to ketones
- (dichromate)
- /pyridine (Collins reagent)
- Chromium pyridinium compound (PCC)
- Dichromate of pyridinium (PDC, Cornforth reagent)
- Periodinane by Dess-Martin
- Oxalyl chloride and dimethyl sulfoxide (DMSO) (Swern oxidation)
/acetone (Jones oxidation)- Acetone with aluminum isopropoxide (Oppenauer oxidation)
To learn more about oxidation of alcohols with the given link
brainly.com/question/7207863
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<u>Question:</u>
Identify the reagents necessary to achieve each of the following transformations
Answer: In order to be alive there must be cells present and since sugar does not contain cells it is not alive.
Explanation:
In this problem, we need to use the ideal gas law. The following is the formula used in ideal gas law: PV = nRT, where n refers to the moles and R is the gas constant.
Given
P = 10130.0 kPa
V = 50 L
T = 300 degree celcius + 273.15 = 573.15 K
R = 8.314 L. kPa/K.mol
Solution
To get the moles which represent the "n" in the formula, we need to rearrange the equation.
PV = nRT PV
---- ------ ---> n = --------
RT RT RT
10130.0 kPa x 50 L
n= ---------------------------------------------
8.314 L. kPa/K.mol x 573.15 K
506,500
= ----------------------------
4,765.17 mol K
=106.29 mol Ar
So the moles of argon gas is 106.29 moles
The chemical reaction of Cavendish involving zinc would be a reaction between hydrochloric acid and zinc yielding zinc chloride and hydrogen gas. The balanced chemical equation would be:
2Zn + 2HCl = 2ZnCl + H2
This is an example of a single replacement reaction where zinc replaces hydrogen in the acid molecule.
Answer:
The sample will be heated to 808.5 Kelvin
Explanation:
Step 1: Data given
Volume before heating = 2.00L
Temperature before heating = 35.0°C = 308 K
Volume after heating = 5.25 L
Pressure is constant
Step 2: Calculate temperature
V1 / T1 = V2 /T2
⇒ V1 = the initial volume = 2.00 L
⇒ T1 = the initial temperature = 308 K
⇒ V2 = the final volume = 5.25 L
⇒ T2 = The final temperature = TO BE DETERMINED
2.00L / 308.0 = 5.25L / T2
T2 = 5.25/(2.00/308.0)
T2 = 808.5 K
The sample will be heated to 808.5 Kelvin
