1. For which of these elements would the first ionization energy of the atom be higher than that of the diatomic molecule?
1 answer:
Answer: Option (b) is the correct answer.
Explanation:
The energy necessary to remove an electron from a gaseous atom or ion is known as ionization energy.
This means that smaller is the size of an atom more amount of energy has to be supplied to it in order to remove the valence electron. This is because in small atom or element there will be strong force of attraction between the nucleus and electrons.
So, high amount of energy has to be supplied to remove the valence electrons.
As electronic configuration of helium is . So, due to completely filled valence shell it is more stable in nature.
As a result, we need to provide very high amount of energy to remove an electron from a helium atom.
Thus, we can conclude that out of the given options helium element would the first ionization energy of the atom be higher than that of the diatomic molecule.
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Answer:
Only II) is correct
Explanation:
I) The red color of the rubies is a physical property of its own structure (wich contains chromium ions)
II)Objects made of silver become tarnished not by a physical property, but as the result of a chemical reaction on the surface of the object made of silver in combination with the sulfur in the air
This changes the color of the object to black, (similar to the iron oxidation)
iii)Boiling is a physical change where a liquid substance absorbs heat in some way (e.g. a flame) and becomes a gas
Answer: The percentage yield of the given reaction is 77.33%.
Explanation:
Moles is calculated by using the formula:
- Moles of Ammonia:
Given mass of ammonia = 150g
Molar mass of ammonia = 17 g/mol
Putting values in above equation, we get:
- Moles of Oxygen
Given mass of oxygen = 150g
Molar mass of oxygen = 32 g/mol
Putting values in above equation, we get:
For the given chemical equation:
By Stoichiometry,
5 moles of oxygen reacts with 4 moles of ammonia.
So, 4.6875 moles of oxygen will react with = of ammonia
As, moles of ammonia required is less than the calculated moles. Hence, ammonia is present in excess and is termed as excess reagent.
Therefore, oxygen is considered as a limiting reagent because it limits the formation of products.
By Stoichiometry of the given reaction:
5 moles of oxygen gas produces 4 moles of nitric oxide
So, 4.6875 moles of oxygen gas will produce = of nitric oxide
Now, to calculate the theoretical amount of nitric oxide, we use equation 1:
Molar mass of nitric oxide = 30 g/mol
Given mass of nitric oxide = 112.5 g
Now, to calculate the percentage yield, we use the formula:
Experimental yield = 87 g
Theoretical yield = 112.5 g
Putting values in above equation, we get:
Hence, the percentage yield of the given reaction is 77.33%.