Question #88b4c

1 Answer
Mar 13, 2017

Answer:

The decrease in mass will be 56.68 g.

Explanation:

The chemical equation and the molar masses are

#M_text(r): color(white)(mmml)286.14color(white)(mmmmmmmmmmmmm)18.02#
#color(white)(mmm)"Na"_2"CO"_3·"10H"_2"O" → "Na"_2"CO"_3·"H"_2"O" + "9H"_2"O"#

Step 1. Calculate the moles of #"Na"_2"CO"_3·"10H"_2"O"#.

#"Moles of Na"_2"CO"_3·"10H"_2"O"#

#= 100.0 color(red)(cancel(color(black)("g Na"_2"CO"_3·"10H"_2"O"))) × ("1 mol Na"_2"CO"_3·"10H"_2"O")/(286.14 color(red)(cancel(color(black)("g Na"_2"CO"_3·"10H"_2"O")))) = "0.3495 mol Na"_2"CO"_3·"10H"_2"O"#

Step 2. Calculate the moles of water released.

#"Moles of H"_2"O" = 0.3495 color(red)(cancel(color(black)("mol Na"_2"CO"_3·"10H"_2"O"))) × ("9 mol H"_2"O")/(1 color(red)(cancel(color(black)("mol Na"_2"CO"_3·"10H"_2"O")))) = "3.145 mol H"_2"O"#

Step 3. Calculate the mass of water released.

#"Mass of water" = 3.145 color(red)(cancel(color(black)("mol H"_2"O"))) × ("18.02 g H"_2"O")/(1 color(red)(cancel(color(black)("mol H"_2"O")))) = "56.68 g H"_2"O"#