How do I dilute 98% sulfuric acid to a 1.0 molar solution?

H2SO4= 98.08 g/mole
98.08 g/.98(98%) = 100.08 g required

Concentrated sulfuric acid (98%) is 18.4 Molar.

Sulfuric acid has a M.W. of 98, density of 1.84 g/mL

You can double check your answer by clicking on the link I have provided, but if you don't try first, you won't learn anything.

And, of course, you add the acid to the water, not the other way around.

1) The mass of 1 mole of sulfuric acid (H2SO4) is 2(1) + 1(32) + 4(16)  = 98 g
2) Find the mass of the concentrated sulfuric acid that contains 98 g of H2SO4.
100g of the concentrated acid is 98% sulfuric acid or contains 0.98 (100) = 98 g
3) Place a clean dry 250 ml beaker on a measuring balance and slowly pour the concentrated acid into the beaker until you have 100 g of concentrated acid. If you overshoot the mass, use an eyedropper to remove the excess.
4) Using a clean dry 1.0L volumetric flask, pour about 600 ml of distilled water into it, SLOWLY pour the concentrated acid into the 600ml of distilled water SWIRLING the flask all the time to distribute the heat formed by the solution process.
5) Pour 100 ml of distilled water into the 250 ml beaker to rinse out the remaining acid and add this to the volumetric flask. Repeat one more time and then add enough distilled water to bring the total volume to 1.0L
6) Cool to room temperature and add more distilled water to make up 1.0L