Answer :
The given problem is based on the chemistry concept of theoretical and actual yield. By calculating the theoretical yield based on molar ratios in the reaction
Comparing it to the actual yield given in the problem, we can conclude that the percentage yield of the product (Sodium chloride or NaCl) in this reaction is approximately 91.5%.
The given question revolves around the concept of theoretical and actual yield, thus classifying it as a topic in Chemistry. The theoretical yield is the maximum amount of product that can be produced in a chemical reaction from a given amount of reactants. The actual yield is the amount of product actually produced in the laboratory during the reaction.
Looking at the reaction, 2 Na + Cl2 --> 2 NaCl, we can see that the molar ratio of sodium (Na) to sodium chloride (NaCl) is 1:1. The atomic weight of sodium (Na) is approximately 23g, so if we have 15.9g of Na and its molar mass is 23g/mol, we get approximately 0.69 moles of Na.
Since the molar ratio of sodium (Na) to sodium chloride (NaCl) is 1:1, theoretically, we should be able to produce 0.69 moles of NaCl. But since the molar mass of NaCl is approximately 58.44g, thus theoretically we can produce: 0.69 moles of NaCl * 58.44 g/mol = approximately 40.32 g of NaCl.
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