A chemist reacted 11.50 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is shown. Na + Cl2 → NaCl

If the percentage yield of the reaction is 85%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors.

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24.65 grams Actual Yield

Explanation:

Given          2Na    +    Cl₂  =>        2NaCl

           11.50g/23g/mol

              = 0.50mole Na >  0.50mole NaCl Theoretical

                                               = 0.50mole NaCl x 58 g/mole

                                               = 29g NaCl Theoretical

Actual Yield = 85% of Theoretical Yield

                     = 0.85 x 29 grams

                     = 24.65 grams Actual Yield

the answer is definitely c.

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3