One atom of an element weighs `1*8xx10^(-22)` g its atomic mass is

Options

A. `29*9`
B. `18`
C. `108*36`
D. `154`

Explanation

To find the atomic mass of the element given that one atom weighs \( 1.8 \times 10^{-22} \) grams, we can follow these steps:

### Step 1: Understand the relationship between atomic mass and the mass of one atom
The atomic mass of an element (in grams per mole) can be calculated using the mass of a single atom and Avogadro's number, which is \( 6.022 \times 10^{23} \) atoms/mole.

### Step 2: Calculate the mass of one mole of atoms
To find the mass of one mole of atoms, we multiply the mass of one atom by Avogadro's number:
\[ \text{Mass of 1 mole of atoms} = \text{mass of 1 atom} \times \text{Avogadro's number} \]
Substituting the values:
\[ \text{Mass of 1 mole of atoms} = (1.8 \times 10^{-22} \text{ g}) \times (6.022 \times 10^{23} \text{ atoms/mole}) \]

### Step 3: Perform the multiplication
Now we will calculate the above expression:
\[ \text{Mass of 1 mole of atoms} = 1.8 \times 6.022 \times 10^{-22 + 23} \]
This simplifies to:
\[ \text{Mass of 1 mole of atoms} = 1.8 \times 6.022 \times 10^{1} \]
Calculating \( 1.8 \times 6.022 \):
\[ 1.8 \times 6.022 = 10.8376 \]
Thus,
\[ \text{Mass of 1 mole of atoms} = 10.8376 \times 10^{1} = 108.376 \text{ g} \]

### Step 4: Round the result
The atomic mass is typically rounded to a reasonable number of significant figures. Therefore:
\[ \text{Atomic mass} \approx 108.36 \text{ g/mol} \]

### Conclusion
The atomic mass of the element is approximately \( 108.36 \) g/mol.

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