Sulfuric acid (h2so4) is prepared commercially from elemental sulfur using the contact process. in a typical sequence of reactions, the sulfur is first burned: s + o2 → so2 , then it is converted to so3 using a catalyst: 2 so2 + o2 → 2 so3 . the resulting so3 is reacted with water to produce the desired product: so3 + h2o → h2so4 . how much sulfuric acid could be prepared from 83 moles of sulfur? answer in units of g.

Explanation:

From the first reaction:

Finding the number of moles using stoichiometry:

Using stoichiometry in the second reaction:

From the third reaction:

Finding the mass in grams of :

the answer for sodium is 0.186

the answer for rubidium is 0.251

chemical digestion occurs in the stomach were hcl and pepsin forms chyme, the mouth in which salivary amylase breaks down starch to form bolus, and the small intestine specifically the duodenum.