find 1. the total no. of neutrons 2. the total mass of neutron in 7mg of C14
Answers
Number of moles in 0.007 g of 14C = mass / molar mass
= 0.007 / 14 = 0.0005 moles
Now 1 mole of 14C = 6.023 X 1023 atoms of 14C
Therefore 0.0005 moles of 14C = 0.0005 X 6.023 X 1023 atoms of 14C
= 3.015 X 1020 atoms of 14C
Now 1 atom of 14C contains 6 protons (atomic number of Carbon is 7).
Therefore there are 8 neutrons present in 1 atom of 14C.
Thus 1 atom of 14C = 8 neutrons
Therefore
3.015 X 1020 atoms of 14C = 8 X 3.015 X 1020 neutrons of 14C
= 2.412 X 1021 neutrons of 14C
Now mass of 1 neutrons = 1.675 X 10-27 Kg
Therefore mass of 2.412 X 1021 neutrons of 14C = 2.412 X 1021 X 1.675 X 10-27 Kg
= 4.04 X 10-6 Kg
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Answer:
Here we have 14C i.e Carbon with mass number = 14
Therefore No of protons + noi of neutrons = 14
Now Atomic no of carbon = No of protons = 6
Therefore No of neutrons are 14 - 6 = 8
Since 14 is the mass no of this isotope of carbon.
That means 14 gram of this carbon will contain 6.02*10^23 ( Avogadro's number) atoms of 14C
Now one atom of 14 C contains 8 neutrons there fore 14 gram of 14C will contain 8 * (6.02*10^23)
That means
14 * 1000 mg ( I gram = 1000 mg) will have 8 * (6.02 * 10^23) neutrons.
14 mg will have [8* (6.02*10^23) ] /1000 = 8 * (6.02 * 10^20)
1 mg = [ 8 * (6.02 * 10^20) ] /14
7 mg = [8 * (6.02 * 10^20) *7 ] / 14
That will be around 24 * 10^20 because you will have to assume Avogadro's number to be 6 * 10^23
So we have Total no of Neutrons equal to 24 * 10^20
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Now We know that mass of a neutron is 1.675 * 10^-27 kg
No of neutrons in 7 mg of 14 C = 24 * 10^20 as we calculated above.
So total mass of neutrons will be [ 1.675*10^-27 ] * [24 * 10^20]
That will be equal to 40.2 * 10^-7 kg