Data and Calculations Don't forget units when recording your values! 33.00g Mass of baking soda (NaHCO:) Mass of the dry NaC:H:O; 3H;0 crystals Description of the appearance of the NACH.O: 3H;0 crystals theoretical yield, in Use the mass of NaHCO, (from the data and calculations section) to calculate moles, of NaCH,Or 3H;0. The theoretical yield of NaC;H,Oz in moles, using the stoichiometry of Reaction 1, is equal to the theoretical yield of the hydrate. moles Theoretical yield of NaC;H,O; 3H:0 136.0779 g/mol What is the molar mass of NaCzHOz: 3H:O? What is theoretical yield of NaC:HsO; 3H;0 in grams? Calculate the percent yield using the following formula: (Mass of dry NaC2H302 3H,0 crystalsy 100% Theoretical yield of NaC,H302 3H20 8.

Data and Calculations Don't forget units when recording your values! 33.00g Mass of baking soda (NaHCO:) Mass of the dry NaC:H:O; 3H;0 crystals Description of the appearance of the NACH.O: 3H;0 crystals theoretical yield, in Use the mass of NaHCO, (from the data and calculations section) to calculate moles, of NaCH,Or 3H;0. The theoretical yield of NaC;H,Oz in moles, using the stoichiometry of Reaction 1, is equal to the theoretical yield of the hydrate. moles Theoretical yield of NaC;H,O; 3H:0 136.0779 g/mol What is the molar mass of NaCzHOz: 3H:O? What is theoretical yield of NaC:HsO; 3H;0 in grams? Calculate the percent yield using the following formula: (Mass of dry NaC2H302 3H,0 crystalsy 100% Theoretical yield of NaC,H302 3H20 8.

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...

See similar textbooks

Similar questions

Balanced chemical reaction between Magnesium hydroxide, with hydrochloric acid. Mg(OH)2(s) + 2 HCl (aq) ➙ MgCl2(aq) + 2 H2O(l) No. Of moles of Mg(OH)2 In 16.1 g :- No. Of moles = mass (g) /molar mass(g) = 16.1 g / 58.32 g/mol = 0.276 moles of Mg(OH)2 is used. No. Of moles of HCl In 11.0 g :- No. Of moles = mass (g) /molar mass(g) = 11.0 g / 36.458 g/mol = 0.302 moles of HCl is used for reaction. According the balance chemical reaction :- 1 mol of magnesium hydroxide require 2 moles of HCl for complete neutralization 0.276 moles of Mg(OH)2 require 0.276 x 2 = 0.552 moles of HCl for complete neutralization, but it is present in less amount. (0.302 moles) Therefore, HCl is the limiting reagent Now, Since HCl is limiting reagent moles of MgCl2 form is depend upon HCl 2 moles of HCl produces 1 mole of MgCl2 0.302 moles of HCl produces ? mole of MgCl2 ? moles of MgCl2 =( 0.302 x 1 )/ 2…
Ff.180.
Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?
2. Write the complete chemical equation for the neutralization of NaOH with HCI. Include states of matter. (2pts) NaOH + HCl +> H,0 t Na cl i.
3. A student mixes 100.0 mL of a 0.100 M solution of potassium phosphate with 100.0 mL of a 0.125 M solution of copper (II) sulfate and obtains a blue solid. (a) Write the balanced chemical equation for the reaction including physical states. (b) Determine the limiting reagent. (c) Calculate the number of moles of the excess reagent after the reaction is completed. Record servation
1. Given the following reaction: (Balance the equation first!) CSHS + 02 --.....-> CO: + H:0 a. If you start with 14.8 g of C;Hy and 3.44 g of Oz, determine the limiting reagent b. Determine the number of moles of carbon dioxide produced c. Determine the number of grams H;O produced d. Determine the number of grams of excess reagent left 2. Given the following equation: Al:Os + Fe --......> Fes04 + Al a. If 25.4 of AlsOs is reacted with 10.2 g of Fe, determine the limiting reagent b. Determine the number of moles of Al produced c. Determine the number of grams of Fe;Os produced d. Determine the number of grams of excess reagent left over in the reaction
Two reaction of interest are as followS: Cl + C,H →C,H,CI + HCI Cl, + C,H→C,HCI, When the reaction is finished, the quantity of each specie is listed below Cl : 160 moles C,H; : 400 moles C,H;Cl : 10 moles C,H;Cl, : 40 moles HCl: 10 moles (a) How many moles of Cl, are there in the feed? (b) How many moles of C,H, are there in the feed? (c) Which one is the limiting reactant? (d) Which one is the excess reactant? (e) What is the %conversion of C,H.? ( What is the selectivity of C. H-Cl relative to C,H,Cl,?
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Cryolite, Na, AIF,(s), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation for the synthesis of cryolite. equation: Al, 0, (s)+NAOH(1)+HF(g) Na, AIF, + H, O(g) If 12.9 kg of Al,0,(s), 56.4 kg of NaOH(1), and 56.4 kg of HF(g) react completely, how many kilograms of cryolite will be produced? mass of cryolite produced: kg Na, AlF, Which reactants will be in excess? NaOH Al, O3 HF What is the total mass of the excess reactants left over after the reaction is complete? total mass of excess reactants: kg Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry | Publisher: University Science Books
If only 3.6 grams of Fe is produced, what is the percent yield of the reaction?
Use the balanced chemical reaction and corresponding reaction map to convert 1.94 moles of Al₂O₃ to moles of Fe.
1. KMnO4, -OH, calor 2. H₂O
3. Consider the following balanced reaction: 2 Fe + 3 Cl₂ → 2 FeCl3 Given 60.0 g of Fe and excess Cl₂ (as much as we need), calculate: a. The theoretical yield of FeCl3, in grams. b. The theoretical amount of Cl₂ consumed, in grams.