## A ring contains 2.4 gram of diamond. How many carbon atoms diamond contains?

A. 3.01×10^23

B. 1.2×10^23

C. 1.2×10^22

D. 1.2×1024

### Answer

Correct Answer: **B. 1.2×10^23 **

### Detailed About MCQs

Use the formula:

N = n *N(A)

In which n = the number of moles, and N(A) is Avogadro’s number, which is 6.02 * 10^23 m^-1.

First of all, the start off by calculating the number of mole Carbon there’s present in the diamond. You got 2.4 grams of the diamond which is made of C atoms. Divide the mass of the diamond with the molar mass of carbon, which is 12.01 g/mole. Hence,

n(C) = 2.4/12.01 = 0.1998 mole

Now, use this formula:

N = n *N(A) => 0.1998 mole * 6,022 * 10^23 mole^-1 = 1.203397169 * 10^23

Hence, the correct answer is Option B.