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. 2.) . Determine your percent yield of sodium chloride in reaction 7.3. Show your work for each step. Write the balanced equation for reaction 7.3 – the reaction between sodium bicarbonate and hydrochloric acid. 3.) Using mass-to-mass stoichiometry, calculate the theoretical yield for reaction 7.3. Use your initial mass of sodium bicarbonate reactant as a starting point, along with the relevant mole ratio from the balanced equation to perform this calculation. Calculate your percent yield of sodium chloride product
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. 2.) . Determine your percent yield of sodium chloride in reaction 7.3. Show your work for each step. Write the balanced equation for reaction 7.3 – the reaction between sodium bicarbonate and hydrochloric acid. 3.) Using mass-to-mass stoichiometry, calculate the theoretical yield for reaction 7.3. Use your initial mass of sodium bicarbonate reactant as a starting point, along with the relevant mole ratio from the balanced equation to perform this calculation. Calculate your percent yield of sodium chloride product
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Question
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.
2.)
. Determine your percent yield of sodium chloride in reaction 7.3. Show your work for each step.
Write the balanced equation for reaction 7.3 – the reaction between sodium bicarbonate and hydrochloric acid.
3.) Using mass-to-mass stoichiometry, calculate the theoretical yield for reaction 7.3. Use your initial mass of sodium bicarbonate reactant as a starting point, along with the relevant mole ratio from the balanced equation to perform this calculation.
Calculate your percent yield of sodium chloride product
Transcribed Image Text:Reaction A: Sodium Bicarbonate and Hydrochloric Acid
Experimental Data
Mass of beaker + watch glass + sodium bicarbonate
Mass of empty beaker + watch glass
Mass of sodium bicarbonate used
Mass of beaker + watch glass + sodium chloride
Mass of sodium chloride collected experimental yield
67.089 g
66.762 g.
0.327g
66.997 g
0.0929
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