Chem $305$

PLEASE HELP WITH THE LAST $3$ QUESTIONS

Lab Exercise #$6-$ Precipitation of $CaC{O}_3$

Data

Mass of $N{a}_{2}C{O}_3$

Mass of $Ca(N{O}_3{)}_2*4H_{2}O$

Mass of unused, marked filter paper

$3$b$)$ Mass of watch glass

Mass of dried filter paper, filtrate, watchglass

$0\mathrm{.}1MNaC{O}_3$ in supernatant observation

$0\mathrm{.}1$MCa$(N{O}_3{)}_2*4H_{2}O$ in supernatant

Data Analysis $($Show your work and put answer on the line.$)$

Calculate the net weight and the number of moles of $CaC{O}_{3(s)}$ that you obtained. Determine the number of moles of each of the starting components. Using your results, determine the percent yield of your reaction.

Molar Mass of $N{a}_{2}C{O}_3$

Molar Mass $ofN{a}_{2}C{O}_3$

$22990(2)+12011+15\mathrm{.}999(3)=10\mathrm{.}9\mathrm{.}988-106$gol

Molar Mass of $Ca(N{O}_3{)}_2*4H_{2}O$

$40\mathrm{.}08+(MiO)+16\mathrm{.}00(3)y^2$

Molar Mass of $CaC{O}_3$

$40\mathrm{.}078+12\mathrm{.}011+3(15\mathrm{.}99a)=\frac{100\mathrm{.}08}{b}ar(6)$

Moles of original $N{a}_{2}C{O}_3$ used in experiment

Mules of original $Ca(N{O}_3{)}_2*4H_{2}O$ used in experiment

Net mass of $CaC{O}_3(s)$ produced in reaction

Chem $305$

Lab Exercise #$6-$ Precipitation of

Moles of $CaC{O}_3(s)$ produced in reaction

$n=\frac{0\mathrm{.}600(g)}{100\mathrm{.}17(mol)}=0\mathrm{.}0059$ or $0\mathrm{.}006$mol

Calculate how many grams of $CaC{O}_3(s)$ you could have produced if ALL of the $N{a}_{2}C{O}_3$ were used up in the reaction

$2\mathrm{.}2264$mol$100\mathrm{.}1\frac{g}{mo},$ Massca $C{O}_3=222\mathrm{.}86g$

Calculate how many grams of $CaC{O}_3(s)$ you could have produced if ALL of the $Ca(N{O}_3{)}_2*4H_{2}O$ were used up in the reaction

$0\mathrm{.}4002md100\mathrm{.}1\frac{\text{m}\text{o}\text{l}}{\text{m}\text{o}\text{l}},$ Mass acon$=40\mathrm{.}06g$

Questions

Which original compound was nearly the limiting reagent in this experiment? Which reagent was the excess reactant in this experiment?

How does your supernatant test support your answer to question #$1?$

Calculate your $\%-$Yield Actual Yield $$ Theoretical Yield