7.R: Mole Ratios and Reaction Stoichiometry (Report)
- Page ID
- 306776
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Reaction A: Sodium Bicarbonate and Hydrochloric Acid
Experimental Data
| Mass of evaporating dish + watch glass (g) | |
|---|---|
| Mass of evaporating dish + watch glass + Sodium bicarbonate | |
| Mass of sodium bicarbonate used | |
| Mass of evaporating dish + watch glass + sodium chloride | |
| Mass of sodium chloride collected (experimental yield) |
Data Analysis
- Use your data to determine the experimental mole-to-mole ratio between sodium bicarbonate and sodium chloride. Show your work for each step.
- Convert the mass of sodium bicarbonate used to moles.
- Convert the mass of sodium chloride collected to moles.
- Divide both of your results from the preceding two steps by the lower mole value to determine the simplest mole-to-mole ratio between sodium bicarbonate and sodium chloride.
- Simplest mole ratio before rounding __________________moles NaHCO3: ________________moles NaCl
- Simplest whole number ratio after rounding ___________________moles NaHCO3: ____________________moles NaCl
- Determine your percent yield of sodium chloride in reaction 3. Show your work for each step.
- Use mass-to-mass stoichiometry, calculate the theoretical yield of NaCl in reaction 3. Use your initial mass of sodium bicarbonate reactant as starting point, along with the relevant mole ratio from the balanced equation to perform this calculation.
- Is your percent yield here for reaction 3 greater than or less than100%? Give one possible source of error that could explain the percent yield you obtained.
Reaction B: Sodium Carbonate and Hydrochloric Acid
Experimental Data
| Mass of evaporating dish + watch glass (g) | |
|---|---|
| Mass of evaporating dish + watch glass + Sodium bicarbonate | |
| Mass of sodium bicarbonate used | |
| Mass of evaporating dish + watch glass + sodium chloride | |
| Mass of sodium chloride collected (experimental yield) |
Data Analysis
- Use your data to determine the experimental mole-to-mole ratio between sodium carbonate and sodium chloride. Show your work for each step.
- Convert the mass of sodium carbonate used to moles.
- Convert the mass of sodium chloride collected to moles.
- Divide both of your results from the preceding two steps by the lower mole value to determine the simplest mole-to-mole ratio between sodium carbonate and sodium chloride.
- Simplest mole ratio before rounding: ___________________moles Na2CO3 ______________________moles NaCl
- Simplest whole number mole ratio after rounding: _________________moles Na2CO3 __________________moles NaCl
- Determine your percent yield in reaction 4. Show your work for each step. Write the balance equation for reaction 4 the reaction between sodium carbonate and hydrochloric acid.
- Using mass-to-mass stoichiometry, calculate the theoretical yield of NaCl for reaction 4. Use your initial mass of sodium carbonate reactant as a starting point, along with the relevant mole ratio from the balanced equation to perform this calculation.
- Is your percent yield here for reaction 4 greater than or less than100%? Give one possible source of error that could explain the percent yield you obtained.