Here’s what I got.
The most important thing to look out for when dealing with a problem is if the chemical equation given to you is balanced. As it turns out, that is not the case here, i.e. your equation is unbalanced.
##”Na”_ 2″S”_ 2″O”_ (3(aq)) + “AgBr”_ ((s)) -> “NaBr”_ ((aq)) + “Na”_ 3[“Ag”(“S”_ 2″O”_ 3)_ 2] “”_ ((aq))##
In order to balance this equation out, you need ##4## atoms of sodium, ##”Na”##, on the reactants’ side. You also need ##2## thiosulfate ions, ##”S”_2″O”_3^(2-)##, on the reactants’ side. You can thus add a ##color(red)(2)## coefficient in front of sodium thiosulfate, ##”Na”_2″S”_2″O”_3##
##color(red)(2)”Na”_ 2″S”_ 2″O”_ (3(aq)) + “AgBr”_ ((s)) -> “NaBr”_ ((aq)) + “Na”_ 3[“Ag”(“S”_ 2″O”_ 3)_ 2] “”_ ((aq))##
Now, the balanced chemical equation tells you that every mole of silver bromide, ##”AgBr”##, that takes part in the reaction consumes ##color(red)(2)## moles of sodium thiosulfate and produces ##1## mole of sodium bromide, ##”NaBr”##.
The problem gives you grams of silver bromide, so right from the start you know that you must convert them to moles by using the compound’s molar mass
##42.7 color(red)(cancel(color(black)(“g”))) * “1 mole AgBr”/(187.77color(red)(cancel(color(black)(“g”)))) = “0.2274 moles AgBr”##
This many moles of silver bromide will consume
##0.2274 color(red)(cancel(color(black)(“moles AgBr”))) * (color(red)(2)color(white)(a)”moles Na”_2″S”_2″O”_3)/(1color(red)(cancel(color(black)(“mole AgBr”)))) = “0.4548 moles Na”_2″S”_2″O”_3##
and produce
##0.2274color(red)(cancel(color(black)(“moles AgBr”))) * “1 mole NaBr”/(1color(red)(cancel(color(black)(“mole AgBr”)))) = “0.2274 moles NaBr”##
Use the molar mass of sodium bromide to convert the number of moles to grams
##0.2274 color(red)(cancel(color(black)(“moles NaBr”))) * “102.9 g”/(1color(red)(cancel(color(black)(“mole NaBr”)))) = color(green)(|bar(ul(color(white)(a/a)color(black)(“23.4 g”)color(white)(a/a)|)))##
You can thus say that the reaction of ##”42.7 g”## of silver bromide produced ##”23.4 g”## of aqueous sodium bromide and consumed
##”no. of moles of Na”_2″S”_2″O”_3 = color(green)(|bar(ul(color(white)(a/a)color(black)(“0.455 moles”)color(white)(a/a)|)))##
of sodium thiosulfate. Both answers are rounded to three , the number of sig figs you have for the mass of silver bromide.
