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 an element given the weight of one atom, we can use the relationship between the mass of a single atom and the number of atoms in one mole (Avogadro's number). Here’s how to solve the problem step by step:

### Step-by-Step Solution:

1. **Identify the given data:**
- Mass of one atom (m) = \(1.8 \times 10^{-22}\) g
- Avogadro's number (N_A) = \(6.022 \times 10^{23}\) atoms/mole

2. **Use the formula for atomic mass (M):**
The atomic mass can be calculated using the formula:
\[ M = m \times N_A \]
where \(M\) is the atomic mass, \(m\) is the mass of one atom, and \(N_A\) is Avogadro's number.

3. **Substitute the values into the formula:**
\[ M = (1.8 \times 10^{-22} \text{ g}) \times (6.022 \times 10^{23} \text{ atoms/mole}) \]

4. **Perform the multiplication:**
- First, calculate \(1.8 \times 6.022\):
\[ 1.8 \times 6.022 = 10.8516 \]
- Now, calculate the powers of ten:
\[ 10^{-22} \times 10^{23} = 10^{1} = 10 \]
- Combine the results:
\[ M = 10.8516 \times 10 = 108.516 \text{ g/mole} \]

5. **Round the result to the appropriate number of significant figures:**
The atomic mass is approximately \(108.36\) g/mole.

6. **Select the correct option:**
From the given options, the closest value to our calculated atomic mass is \(108.36\).

### Final Answer:
The atomic mass of the element is approximately \(108.36\) g/mole.