StoichiometryInstructions: Complete the following questions and hand in at the start of your lab period or wheninstructed by your instructor. Show your work with units and correct significant figures for all questionsthat involve a calculation.1.Calculate the molecular weights of all the compounds in the reaction we are doing in this lab(and copy them onto your procedure... they will be helpful!):a.NaHCO3b. HCIc. NaCld. H₂Oe. CO22. The following is some example data for the lab. Use the data to answer the following questions.Mass of test tube and boiling chipMass of test tube, boiling chip and NaHCO3Mass of test tube, boiling chip and NaCla. How much NaHCO3 was added to the test tube?14.123 g14.724 g14.496 gb. How many grams NaCl was produced from the experiment?c. Using the balanced chemical equation, the amount of limiting reactant calculated above,and molar masses from question 1, how many moles of NaCl should the experiment haveproduced?d. Calculate the percent yield for this experiment.

1. Given: MNa=22.99g/mol;MH=1.01g/mol;MC=12.01g/mol;MO=16.00g/molMCl=35.45g/molStep 1: Solve…

Answered: Stoichiometry Instructions: Complete…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 5CR

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Post-Lab Questions 1. Discuss how each of the following actions would affect the calculated % oxygen in the magnesium oxide compound. Would the percentage be too high, too low, or remain the same? a. The evaporation of water caused "spattering." tion b. Water was not completely removed by evaporation. 2. The white powder often found on objects made of aluminum is aluminum oxide, Al,O, A 5.00 g strip of aluminum is reacted in air, producing an oxide weighing 9.36 g. Calculate the percent oxygen and aluminum in the compound. 3. Aluminum oxide has the empirical formula of Al,O3. a. Calculate the % aluminum in Al,O3, using the chemical formula. b. Calculate the % error for the percent aluminum calculated in question 2. 85 COPYRIGHT 2013 Cengage Learning
7. Use the reaction given to solve the next problems. Show all units. Al203 + 6Na ---> 3Nª2O +2Al a. 2 moles of Al203 will produce. moles of Al. Show all units, b. 5 moles of Na will require. moles of Al203. Show all units. c. 23.0 grams of sodium will produce moles of Na20. Show all units. d. 69.0 grams of sodium will produce grams of Al. Show all units. e. 24.6 moles of aluminum oxide will produce grams of sodium oxide. Show all units. f. 15.3 grams of Na2O will be produced by moles of sodium. Show all units.
DATA: Data Table 1: NaHCO, Reaction Data Mass of evaporating dish (g) 43.9449 g Mass of evaporating dish + NaHCO3 (g) 44.2376 g Mass of NaHCO3 (g) 0.2927 44.1411 g Mass of evaporating dish + NaCl product after 1st heating (g) Mass of evaporating dish + NaCl product after 2nd heating (g) Mass of evaporating dish + NaCl product after 3rd heating (g) (if necessary) Mass of NaCl product (g) (actual yield) 44.1401 g
Endow Help eq req Ereg Important values if needed... | b... q eq MAY 11 Submit Answer prod01-cnow-owl.cengagenow.com S 5 According to the following reaction, how many moles of bromine monochloride will be formed upon the complete reaction of 0.915 moles bromine with excess chlorine gas? Br2(g) + Cl₂ (g) → 2BrCI(g) mol bromine monochloride Retry Entire Group ty A 6 [Review Topics] [References] Use the References to access important values if needed for this question. Module 2 | OWLv2 MacBook Pro & 7 8 more group attempts remaining GA * CO 8 A :)) O 9 COWLV2 | Online teaching and learning resource from C.... Previous 00 Email Instructor Thu May 11 Next Save and Exit 0 HARB 0 + C ?
alibri (Body) 12 A A Aa v AaBbCcDc AaBbCcDc AaBbC AABBCCC AaB AABBCCD IU abe x, x A ab T Normal T No Spac. Heading 1 Heading 2 Title Subtitle Font Paragraph Styles 3 6 IZICIt iniED 10 11 12 13 I 14 I- 15 16 . Chemical Equation Write a balanced equation that describes each of the following chemical reaction. 1. Acetylene gas, C2H2, burns in air forming gaseous carbon dioxide and, CO2, and water. Answer: 2C2H2 + 502 → 4CO2 + 2H20 (double displacement/Combustion reaction) 2. MnO2 + KOH + O2 → H20 + K2MNO4 3. FeCl2 + Cl2 → FeCl3 English (United States) Accessibility: Good to go a ENG REDMI NOTE 10 PRO | JHANG 01/06/2022 15: 12
M Apple Google Disney ESPN Yahoo! Biomedical Careers Program ☆ For the reaction Fe(s) +2HCl(aq)→→→→→FeCl₂(s) + H₂(g) AH° = -7.4 kJ and AS° = 107.9 J/K B Submit Answer Apple ☆ prod03-cnow-owl.cengagenow.com iCloud Yahoo Images Bing Google Wikipedia Facebook Twitter LinkedIn G b COWLv2... b D2L D2L D2L [Review Topics] [References] Use the References to access important values if needed for this question. D2L The maximum amount of work that could be done when 2.08 moles of Fe(s) react at 286 K, 1 atm is Assume that AH° and AS° are independent of temperature. Retry Entire Group 4 more group attempts remaining The Weather Channel C D2L Yelp TripAdvisor M kJ. +
CALCULATIONS: SHOW COMPLETE "SET-UPS" (and the rounding off) for all calculations on the bottom of this a separate sheet. Use the correct number of significant figures and correct units. page or on 1. Mass of PbCrO4 formed 2. Moles of PbCrO4 formed 3. Formula of Limiting Reagent 4. Moles of PbCrO4 predicted by calculation 5. % Difference in moles formed and predicted gnificant figures and correct units. B 44.1248 44.3198 44.2921 A 44.0432 44.3279 14.25979 th both reagents. Briefly, indicate the B
1. Moles of NaHCO3 and NaCl:2. Mole Ratio:3. How does your experimental ratio compare to the theoretical? If they are different,explain what might have caused the difference.4. Calculate the percent error.
The weight of saturated NaCl was obtained by weighing the collected solid. Was thisan accurate weight of saturated NaCl present in the original sample? Explain youranswer.
Bookmarks Window Help 14 Q A Fri De A prod01-cnow-owl.cengagenow.com Bb Content E OWLV2 | Online teaching and learning resource from Cengage Paraphrasing ..ewriting Tool Car note CAU EMAIL CANVAS Pirate Ship MYJSCC BLACKBOARD Vacancies | A.| Birmingham New NCOER C.e Measures [References) Calculate the composition of the gaseous mixture obtained when 4.05 mol of carbon dioxide is exposed to hot carbon at 850°C in a 4.15 L vessel. The equilibrium constant K. ' at 850°C is 1.67 for the reaction CO2(9) + C(s) = 2C0(g) [CO2] = [CO] = Submit Answer Try Another Version 3 item attempts remaining pt pt Next étv 10 MacBook Air DII DD 80 888 F9 F7 F6 FS F2 F3 & @ 23 $ 7 8 2 3 4. Y U W E J K L H S V B M .. .- V R
B. Formula of a Hydrate 23.43 29.24 26.31 26.28 1. Mass of crucible 2. Mass of crucible and hydrate 3. Mass of crucible and anhydrate 3a. Mass of crucible and anhydrate (second heating) Calculations 4. Mass of hydrate 5. Mass of anhydrate 6. Mass of water lost
composition of water in a hydrate, we need to look at our equation. compare it to your experimental values you just obtained in lab. To calculate the percent In this exercise, we are going to calculate the percent composition of water in a hydrate and percent (%) composition = of water mass of water х 100 mass of entire hydrate For LINO3 3H2O (lithium nitrate trihydrate) we have to calculate the mass of each element. Nelice the three in front of the water will give us a total of six hydrogens and three oxygens. Li: 1x 6.94 g/mol N: 1x 14.01 g/mol H: 6x 1.01 g/mol О: 3х 16.00 g/mol O: 3x 16.00 g/mol 54.06 g/mol go l00 68.95 g/mol percent (%) composition = of water 3 H20 х 100 LINO3 · 3H20 percent (%) composition = of water 54.06 g/mol х 100 (68.95 g/mol + 54.06 g/mol) percent (%) composition of water in LINO3 • 3 H20 = 43.9 % 1. Calculate the percent composition of water in the following hydrates: (show all work) ZnSO, 7H20 M9SO 7H20 BaCl2 2H20 There are additional questions on the…

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