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

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

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