A naturally occuring sample of copper consists of 69.2% of $^{63} C u$ and 30.8% of $^{65} C u$ . The relative mass of $^{63} C u$ is 62.93 and that of $^{65} C u$ is 64.93. Find the atomic mass of a naturally occuring sample of copper.

64.348

No worries! We‘ve got your back. Try BYJU‘S free classes today!

63.546

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

64.12

No worries! We‘ve got your back. Try BYJU‘S free classes today!

none of these

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B 63.546
The atomic mass of $C u^{63}$ is 62.93 and relative abundance = 69.2%
The atomic mass of $C u^{65}$ is 64.93 and relative abundance = 30.8%
Therefore, relative atomic mass of Cu = $\frac{(62.93 \times 69.2) + (64.93 \times 30.8)}{100} = 63.546$

Suggest Corrections

Similar questions

C u

has only two naturally occurring isotopes,

63_{C u}

and

65_{C u}

. If the atomic mass of

C u

63.546

, then the natural abundance of the

^{63} C u

isotope will be approximately :

1)copper has two naturally occurring isotopes copper 63 has an atomic mass of 62. 9 296 u and an abundance of 69. 1 5% what is the atomic mass of the second isotopic if the average atomic weight of copper is 63?

Q. The average mass of one gold atom in a sample of naturally occurring gold is

3.257 \times 10^{- 22} g

. Using this, the molar mass of gold calculated is :

Q. The average mass of one gold atom in a sample of naturally occurring gold is

3.27 \times 10^{- 22}

g. Calculate the molar mass of gold. (Nearest integer)

Q. Boron occurs in nature in the form of two isotopes having atomic mass 10 and 11. Calculate the percentage abundances of two isotopes respectively in a sample having atomic mass 10.80.

Join BYJU'S Learning Program

A naturally occuring sample of copper consists of 69.2% of 63Cu and 30.8% of 65Cu. The relative mass of 63Cu is 62.93 and that of 65Cu is 64.93. Find the atomic mass of a naturally occuring sample of copper.

The correct option is B 63.546The atomic mass of Cu63 is 62.93 and relative abundance = 69.2%The atomic mass of Cu65 is 64.93 and relative abundance = 30.8%Therefore, relative atomic mass of Cu = (62.93×69.2)+(64.93×30.8)100=63.546

A naturally occuring sample of copper consists of 69.2% of $^{63} C u$ and 30.8% of $^{65} C u$ . The relative mass of $^{63} C u$ is 62.93 and that of $^{65} C u$ is 64.93. Find the atomic mass of a naturally occuring sample of copper.

The correct option is B 63.546
The atomic mass of $C u^{63}$ is 62.93 and relative abundance = 69.2%
The atomic mass of $C u^{65}$ is 64.93 and relative abundance = 30.8%
Therefore, relative atomic mass of Cu = $\frac{(62.93 \times 69.2) + (64.93 \times 30.8)}{100} = 63.546$