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 11.7 grams of HCl (36.5 g/mol) react with excess NaOH and 17.5 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?
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 11.7 grams of HCl (36.5 g/mol) react with excess NaOH and 17.5 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?
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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 11.7 grams of HCl (36.5 g/mol) react with excess NaOH and 17.5 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?
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