Sulfuric acid is purchased full-strength at 18.0M. How many milliliters of full-strength acid are needed to prepare 500.0 mL of aqueous 0.35M H2SO4? Round your answer to 3 significant figures. A. 13.4 mL
B. 82.6 mL
C. 9.70 mL
D. 79.0 mL

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

the answer for sodium is 0.186

the answer for rubidium is 0.251

answer: they produce more slow than unicellular organisms.