CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon


Question

The isotopic abundance of C-12 and C-14 is 98% and 2% respectively. What would be the number of C - 14 isotope in 12 g carbon sample?


A
1.032×1022
loader
B
3.01×1023
loader
C
5.88×1023
loader
D
6.02×1023
loader

Solution

The correct option is D $$1.032\, \times\, 10^{22}$$
Isotopic abundance of $$C-12$$ is $$98$$%
Isotopic abundance of $$C-14$$ is $$2$$%
Average atomic mass $$= \cfrac {Mass \ number \times Relative \ abundance \ + \ Mass \ number \times Abundance}{100}$$
$$= \cfrac {98 \times 12 + 2 \times 14}{100}$$
$$=12.04 \ grams$$
So, in $$100$$ grams of carbon sample, $$C-14$$ isotope will be $$2$$ grams since it is $$2$$% in abundance.
$$\therefore$$ in $$12$$ grams sample, $$C-14$$ isotope will be $$=\cfrac {12 \times 2}{100}=0.24 \ grams$$
$$1$$ mole of any compound has $$N_A$$ number of atoms i.e $$6.02 \times 10^{23}$$. 
So, $$C-14$$ isotope will be $$1.032 \times 10^{22}$$

Chemistry

Suggest Corrections
thumbs-up
 
0


similar_icon
Similar questions
View More


similar_icon
People also searched for
View More



footer-image