Question #c4ab3
1 Answer
Explanation:
Start by writing the balanced chemical equation that describes this double replacement reaction
#"AgNO"_ (3(aq)) + "NaCl"_ ((aq)) -> "AgCl"_ ((s)) darr + "NaNO"_ (3(aq))#
The reaction consumes sodium chloride and silver nitrate in a
#overbrace("moles of NaCl = moles of AgNO"_3)^(color(blue)("consumed by the reaction")) = overbrace("moles of AgCl")^(color(blue)("produced by the reaction"))#
Use the molar mass of sodium chloride to convert the mass to moles
#53.7648 color(red)(cancel(color(black)("g"))) * "1 mole NaCl"/(58.44color(red)(cancel(color(black)("g")))) = "0.9200 moles NaCl"#
Since silver nitrate is in excess, you can say that at
To convert the number of moles to grams, use the molar mass of silver chloride
#0.9200 color(red)(cancel(color(black)("moles AgCl"))) * "143.32 g"/(1color(red)(cancel(color(black)("mole AgCl")))) = "131.8544 g"#
However, you know that the reaction produced
To find the percent yield of the reaction, calculate the mass of silver chloride produced for every
#100 color(red)(cancel(color(black)("g in theory"))) * "90.42919 g produced"/(131.8544color(red)(cancel(color(black)("g in theory")))) = "68.5826 g"#
Therefore, you can say that the reaction will have a percent yield of
#color(darkgreen)(ul(color(black)("% yield" = 68.5826%)))#
The answer is rounded to six sig figs, the number of sig figs you have for the mass of sodium chloride.