If 3.01 × 1020 molecules are removed from 98 mg of H2SO4 , then the number of moles of H2SO4 left are 0.1 × 10–3 0.5 × 10–3 1.66 × 10–3 9.95 × 10–2

The question seems to be incomplete. However, I can guide you on how to approach this problem.

1. First, you need to know the molar mass of H2SO4, which is approximately 98 g/mol.

2. Then, convert the given mass (98 mg) of H2SO4 to grams by dividing by 1000 (since 1g = 1000mg), which gives 0.098 g.

3. Convert this mass to moles by dividing by the molar mass. So, the number of moles of H2SO4 initially present is 0.098 g / 98 g/mol = 0.001 mol.

4. Now, you need to find out how many moles of H2SO4 are represented by 3.01 × 10^20 molecules. Use Avogadro's number (6.022 × 10^23 molecules/mol) for this. So, the number of moles of H2SO4 removed is 3.01 × 10^20 molecules / 6.022 × 10^23 molecules/mol = 0.0005 mol.

5. Subtract the number of moles removed from the initial number of moles to find the number of moles left. So, the number of moles of H2SO4 left is 0.001 mol - 0.0005 mol = 0.0005 mol.

Please note that the question seems to be incomplete and the provided options do not match the calculated answer. Please check the question again.