when 20ml,N/5 HCL reacts with 40mg of Na2Co3 then find the limiting reagent and weight of co2 formed?
Answers
Answer:
Objectives and Background
The objectives of this laboratory are to experimentally determine the mole-to-mole ratios between the
underlined reactants and products in the following two double displacement “gas forming” reactions:
(A) sodium bicarbonate + hydrochloric acid → sodium chloride + carbon dioxide + water
(B) sodium carbonate + hydrochloric acid → sodium chloride + carbon dioxide + water
The easiest way to obtain the mole-to-mole ratios would be to simply balance the chemical equations for
these reactions. This would be considered a theoretical approach to the problem. The balanced
equations for reactions A and B are:
(A) 1 NaHCO3 (s) + 1 HCl (aq) → 1 NaCl (aq) + 1 CO2 (g) + 1 H2O (l)
(B) 1 Na2CO3 (s) + 2 HCl (aq) → 2 NaCl (aq) + 1 CO2 (g) + 1 H2O (l)
In reaction A, the balancing coefficients indicate that there is a 1:1 mole ratio between reactant NaHCO3
and product NaCl. This means that for every 1 mole of sodium bicarbonate that reacts, 1 mole of
sodium chloride should be produced. However in reaction B, the balancing coefficients indicate that
there is a 1:2 mole ratio between reactant Na2CO3 and product NaCl. In this case, for every 1 mole of
sodium carbonate that reacts, 2 moles of sodium chloride should be produced.
To determine these mole-to-mole ratios experimentally, a quantitative analysis of both reactions is
required. Specifically, a pre-weighed mass of sodium bicarbonate/carbonate will be allowed to react
with a slight excess of hydrochloric acid. The sodium chloride product will then be carefully retrieved,
dried and weighed at the end of the reaction. This mass of collected sodium chloride is called an
experimental yield. Both the mass of sodium bicarbonate/carbonate reactant used and the mass of
sodium chloride product can be converted to mole quantities via their respective molar masses. Finally,
dividing both the reactant and product moles by the lower of the two values should yield the simplest
whole number mole-to-mole ratio of reactant and product.
While an experimental product yield is obtained by actually performing a reaction in lab, a theoretical
yield is the maximum mass of product that could be obtained from a reaction provided that no errors
occur. Theoretical product yields can only be determined by performing a series of stoichiometric
calculations. Thus, using this method, theoretical yields of sodium chloride will be calculated for
reactions A and B. Once obtained, the percent yield of sodium chloride can be determined for both
reactions, where
Percent Yield =
Experimental Yield
Theoretical Yield X 100
Good experimental practices in the lab (with minimum error) generally result in a high percent yield,
where the experimental yield closely approaches the theoretical yield.
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