Use data given in the following table to calculate the molar mass of naturaly occuring argon isotopes:
`{:("Isotope",,"Isotopic molar mass",,"Abundance"),(.^(36)Ar,,35.96755 g mol^(-1),,0.337%),(.^(38)Ar,,37.96272 g mol^(-1),,0.063%),(.^(40)Ar,,39.9624 g mol^(-1),,99.600%):}`
(Round of the answer to the nearest whole number ).

Explanation

To calculate the molar mass of naturally occurring argon isotopes, we will use the formula for the average atomic mass based on the isotopic molar masses and their respective abundances. Here are the steps:

### Step-by-Step Solution:

1. **Identify the Isotopes and Their Data**:
- Isotope \( ^{36}Ar \): Isotopic molar mass = 35.96755 g/mol, Abundance = 0.337%
- Isotope \( ^{38}Ar \): Isotopic molar mass = 37.96272 g/mol, Abundance = 0.063%
- Isotope \( ^{40}Ar \): Isotopic molar mass = 39.9624 g/mol, Abundance = 99.600%

2. **Convert Abundances from Percent to Decimal**:
- For \( ^{36}Ar \): \( 0.337\% = \frac{0.337}{100} = 0.00337 \)
- For \( ^{38}Ar \): \( 0.063\% = \frac{0.063}{100} = 0.00063 \)
- For \( ^{40}Ar \): \( 99.600\% = \frac{99.600}{100} = 0.99600 \)

3. **Calculate the Contribution of Each Isotope to the Average Atomic Mass**:
- Contribution from \( ^{36}Ar \):
\[ 35.96755 \, \text{g/mol} \times 0.00337 = 0.12163 \, \text{g/mol} \]
- Contribution from \( ^{38}Ar \):
\[ 37.96272 \, \text{g/mol} \times 0.00063 = 0.02392 \, \text{g/mol} \]
- Contribution from \( ^{40}Ar \):
\[ 39.9624 \, \text{g/mol} \times 0.99600 = 39.87074 \, \text{g/mol} \]

4. **Sum the Contributions**:
\[ \text{Total Average Atomic Mass} = 0.12163 + 0.02392 + 39.87074 = 39.01629 \, \text{g/mol} \]

5. **Round Off to the Nearest Whole Number**:
\[ \text{Average Atomic Mass} \approx 39 \, \text{g/mol} \]

### Final Answer:
The molar mass of naturally occurring argon isotopes is approximately **39 g/mol**.