Which of the following is a characteristic of the actinides?
1 answer:
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Answer:
(CH3)2CHCH2CHO
Explanation:
The reaction sequence begins with the reaction of isopropanol with phosphorus tribromide to yield isopropyl bromide. This is followed by reaction with Magnesium in ether solution giving a grignard reagent, isopropyl magnesium bromide. This is now attacked by oxirane and the epoxide ring opens, hydrolysis of the product, followed by oxidation using pyridinium chlorochromate (PCC) yields the final product- (CH3)2CHCH2CHO
The detailed reaction mechanism is attached to this answer.
Answer:
- The molar mass of the solute, in order to convert from moles of solute to grams of solute.
- The density of solution, to convert from volume of solution to mass of solution.
Explanation:
Hello,
In this case, since molarity is mathematically defined as the moles of solute divided by the volume of solution and the weight/weight percent as the mass of solute divided by the mass of solution, we need:
- The molar mass of the solute, in order to convert from moles of solute to grams of solute.
- The density of solution, to convert from volume of solution to mass of solution.
For instance, if a 1-M solution of HCl has a density of 1.125 g/mL, we can compute the w/w% as follows:
Whereas the first factor corresponds to the molar mass of HCl, the second one the conversion from L to mL of solution and the third one the density to express in terms of grams of solution.
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<u>Answer:</u> The molar solubility of nitrogen gas when pressure is increased is 0.042 mol/L
<u>Explanation:</u>
We are given:
Solubility of nitrogen gas in water = 56.0 mg/100 g
Or, solubility of nitrogen gas in water = 0.056 g/100 mL (Density of water = 1 g/mL & Conversion factor used: 1 g = 1000 mg)
Solubility of a solute is defined as the moles of solute dissolved in 1 L of solvent.
Conversion factor used: 1 L = 1000 mL
Applying unitary method:
In 100 mL water, the amount of solute (nitrogen gas) dissolved is 0.056 grams
So, in 1000 mL of water, the amount of solute (nitrogen gas) dissolved will be =
Converting this solubility into mol/L by dividing with the molar mass of nitrogen gas:
Molar mass of nitrogen gas = 28 g/mol
So, Solubility of nitrogen gas =
To calculate the Henry's constant we use the equation given by Henry's law, which is:
.........(1)
where,
= Henry's constant
= molar solubility of nitrogen gas = 0.02 mol/L
= partial pressure of nitrogen gas = 2.38 atm
Putting values in equation 1, we get:
<u>When pressure is changed to 5.00 atm</u>
Now,
Putting values in equation 1, we get:
Hence, the molar solubility of nitrogen gas when pressure is increased is 0.042 mol/L