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35710 3 46510 3 46510 3 46510 3 081 or 11 ratio

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3.57*10-3:4.65*10-3/ 4.65*10-3: 4.65*10-3= 0.8/1 or 1:1 ratioSimplest mole ratiobeforerounding___________0.8______________________ moles NaHCO3: __________________1_________ moles NaClSimplest whole number mole ratioafterrounding_______1__________________________ moles NaHCO3: __________1_________________ moles NaCl2)Determine your percent yield of sodium chloride in reaction A.Show your work for each step.Page 1of 3
●Write the balanced equation for reaction A – the reaction between sodium bicarbonate and hydrochloric acid.2(g)
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●Using mass-to-mass stoichiometry, calculate the theoretical yield of NaCl for reaction A. Use your initialmass of sodium bicarbonate reactant as a starting point, along with the relevant mole ratio from thebalanced equation to perform this calculation.
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●Calculate your percent yield of sodium chloride product.
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Reaction B: Sodium Carbonate and Hydrochloric AcidExperimental Data(a) Mass of evaporating dish + watch glass47.731 g(b) Mass of evaporating dish + watch glass + sodium carbonate48.031 g(c) Mass of sodium carbonate used0.300 g(d) Mass of evaporating dish + watch glass + sodium chloride48.141 g
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