Explanation:
The given data is as follows.
Energy needed for 1 mole = 279.7 kJ = 
= 279700 J
Therefore, energy required for 1 atom will be calculated as follows.
= 
As relation between energy and wavelength is as follows.
E = 
where, h = planck constant = 
c = speed of light = 
= wavelength
Therefore, putting given values into the above formula as follows.
E =
= 
= 
or, = 
m
= 428 nm
Thus, we can conclude that the maximum wavelength of light that can remove an electron from an atom on the surface of lithium metal is 428 nm.
The third one is the correct answer :)
Answer:- 71.7 calories
Solution:- it is a unit conversion problem where we need to convert joules into calories.
The unit conversion for these energy units is:
1 calorie = 4.184 joule
The given energy is 300 joules and has to be converted to calories. We will show the set up using dimensional analysis.
= 71.7 calories
So, the energy in calories is 71.7.
Answer:
in the attached image is the reaction mechanism.
Explanation:
The first reaction (reaction 1) shown in the attached image is the Wolff-Kishner reduction, which is characterized when the carbonyl is reduced to an alkane in the presence of a hydrazine and a base. In reaction 1, the aldehyde reacts with hydrazine to produce oxime. This mechanism begins with the attack of the amine on the carbonyl group. Proton exchange happens and the water leaves the molecule.
In reaction 2, the KOH is deprotoned in nitrogen and organized to form the bond between the nitrogen molecule. this deprotonation releases the nitrogen gas
