Lets say we are given this balanced equation: #CaO + 2HCl -> CaCl_2 + H_2O#. 60.4g of #CaO# is reacted with 69.0g of #HCl#. How much #CaCl_2# is produced?
1 Answer
Explanation:
Start by writing out the balanced chemical equation that describes your reaction
#"CaO"_ ((s)) + color(red)(2)"HCl"_ ((aq)) -> "CaCl"_ (2(aq)) + "H"_ 2"O"_ ((l))#
You need
You an convert this mole ratio to a gram ratio by using the molar masses of the two compounds
#M_("M CaO") = "56.08 g mol"^(-1)#
#M_("M HCl") = "36.46 g mol"^(-1)#
A
#(56.08 color(red)(cancel(color(black)("g mol"^(-1)))))/(color(red)(2) * 36.46color(red)(cancel(color(black)("g mol"^(-1))))) = 56.08/72.92 -># gram ratio
So, you need
You know that you have a sample of
#60.4 color(red)(cancel(color(black)("g CaO"))) * "72.92 g HCl"/(56.08color(red)(cancel(color(black)("g CaO")))) = "78.54 g HCl"#
Since you have less hydrochloric acid than you would need in order for all the mass of calcium oxide to react
#overbrace("69.0 g")^(color(blue)("what you have")) < overbrace("78.54 g")^(color(darkgreen)("what you need"))#
you can conclude that hydrochloric acid will act as a limiting reagent, i.e. it will be completely consumed before all the grams of calcium oxide get a chance to react.
Use the molar mass of calcium chloride to convert the
#M_("M CaCl"_2) = "111.0 g mol"^(-1)#
You will have
#(color(red)(2) * 36.46 color(red)(cancel(color(black)("g mol"^(-1)))))/(111.0color(red)(cancel(color(black)("g mol"^(-1))))) = 72.92/111.0 -># gram ratio
Since all the hydrochloric acid will react, you can say that the reaction will produce
#69.0 color(red)(cancel(color(black)("g HCl"))) * "111.0 g CaCl"_2/(72.92color(red)(cancel(color(black)("g HCl")))) = color(green)(|bar(ul(color(white)(a/a)color(black)("105 g CaCl"_2)color(white)(a/a)|)))#
The answer is rounded to three sig figs.