One important factor in any chemical synthesis is the actual quantity of desired product obtained compared to the theoretical amount predicted on the basis of the stoichiometry of the reaction. the ratio of the mass of product obtained to the theoretical quantity, expressed as a percentage, is referred to as the "percent yield" or more simply the "yield". for example: if we react hcl with excess naoh one of the products will be nacl. if we assume that all of the cl in hcl ends up as nacl we know that each mole of hcl consumed should produce a mole of nacl product. suppose that in a particular reaction 10.9 grams of hcl (36.5 g/mol) react with excess naoh and 19 grams of nacl (58.5 g/mol) are isolated from the reaction mixture by crystallization. what is the percent yield of nacl in the experiement?

the percent yield of NaCl in the experiement is 109%.

Explanation:

1) Each mole of HCl consumed should produce a mole of NaCl product

  ⇒ 1 mol HCl / 1 mol NaCl

2) Reactant: 10.9 grams of HCl (36.5 g/mol)

3) Theoretical (stoichiometric) yield of NaCl

        ⇒ x = 0.299 mol NaCl (should be obtained)

4) Actual yield

5) Percent yield:

Note: it is not normal to obtain percent yields greater than 100%.  When this happens, you must think in an experimental error or that the sample was contaminated with some substance that yield to an increase of the measured product.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.

answer carbon and three oxygen atoms;