Question

On a conventional scale, the atomic weight of sulfur is \[32\] . If on a new scale, an amu is defined as one-third by weight of an atom of \[C - 12\] isotope, what would be the atomic weight of sulphur on this new scale?

Answer 1

Hint: To solve this question, we must first calculate the atomic weight of sulfur on a new scale using the weight of an atom of \[carbon - 12\] isotope in new scale and atomic weight of sulfur in conventional scale. Then we need to assess the formula for the calculation and then only we can conclude the correct answer.

Complete step by step answer:
Before we move forward with the solution of this given question, let us first understand some basic concepts:
We can define the equivalent weight of an element as the atomic weight divided by outermost electrons in compounds. Atomic mass unit is the unit of equivalent weight of an element, the amount of substance in gram is same to the equivalent weight called as the gram equivalent weight.
Here, a.m.u stands for atomic mass unit, which is the mass of an atom.
 Step 1: In this step we will enlist the given quantities:
Atomic weight of sulfur $ = 32$
The mass of carbon $ = 12$
Step 2: In this step we will calculate the atomic weight of sulphur on this new scale:
Suppose, the atomic weight of sulfur in the new scale as x.
One amu is one-third by weight of an atom of \[carbon - 12\] isotope. So, let us now calculate the atomic weight of sulfur in new scale as:
$
\frac{1}{3} \times x \times 12 = \,\,32 \\
\Rightarrow \,\,4x = \,\,32 \\
\Rightarrow x = 8 \\
$
So, the atomic weight of sulfur in the new scale is $8$ . And hence, this is the required answer.

Note:All living things need sulphur. It is especially important for humans because it is part of the amino acid methionine, which is an absolute dietary requirement for us. The amino acid cysteine also contains sulphur. The average person takes in around 900 mg of sulphur per day, mainly in the form of protein.