Record all masses to the maximum number of Run 1 Run 2 sig figs 200°C 400°C 1. Mass of beaker 81.061 27.986 2. Mass of beaker + NaHCO3 85.457 32.267 3. Initial mass of NaHCO3 4.476 4.292 Mass of beaker plus products after heating. 4. 84.3 80 30.742 5. Mass of product (actual yield) There are three theoretically possible chemical reactions that could occur during the thermal decomposition of baking soda. 1) sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g) 2) sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g) 3) sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g)

Record all masses to the maximum number of Run 1 Run 2 sig figs 200°C 400°C 1. Mass of beaker 81.061 27.986 2. Mass of beaker + NaHCO3 85.457 32.267 3. Initial mass of NaHCO3 4.476 4.292 Mass of beaker plus products after heating. 4. 84.3 80 30.742 5. Mass of product (actual yield) There are three theoretically possible chemical reactions that could occur during the thermal decomposition of baking soda. 1) sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g) 2) sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g) 3) sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g)

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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A. Calculate the moles of anhydrous (dry) KAl(SO4)2 that were present in the sample. Step 1: Find the mass of the dry anhydrous salt show work: Final weighing - mass of pan = mass of anhydrous salt Step 2: Find the molar mass of KAl(SO4)2 and show work here Step 3: Find the moles with work shown: grams of the dry salt divided by the molar mass = moles B. Calculate the ratio of moles of H2O to moles of anhydrous KAl(SO4)2. Note: Report the ratio to the closest whole number. Show work here: Take the value of the moles of water and divide by the moles of the salt. Round to the nearest whole number C. Write the empirical formula for the hydrated alum, based on your experimental results and answer to Question B. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(S04)2•4H20. Show your work. the image uploaded is the table that is needed to answer these questions
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Al reacts with hydrochloric acid according to the following balanced equation: 2 Al + 6 HCl ==> 2 AlCl3 + 3 H2 What mass of Al is required to produce 32.67 g of hydrogen gas? Give your answer to 2 decimal places. Molar Mass, g/mol Al 26.98 HCl 36.46 AlCl3 133.34 H2 2.016
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Carbon dioxide gas reacts with dihydrogen monoxide, producing carbon tetrahydride gas and oxygen gas. When 60.0 g of carbon dioxide reacts with excess dihydrogen monoxide, the actual yield of oxygen gas is reported as 102 g. a. What is the percent yield of oxygen gas? Show work for full credit. b.Is this yield acceptable, yes or no? Explain why or why not in five sentences or less.
Liquid octane (CH₂(CH₂) CH₂ 6 (CH₂(CH₂) CH₂) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). What is the theoretical yield of water formed from the reaction of 18.3 g of octane and 110. g of oxygen gas? Round your answer to 3 significant figures. g x10 X S
个 app.101edu.co STARTING AMOUNT esc q X 2 #3 3 How many grams of AgCl will be formed when 60.0 ADD FACTOR x( ) completely reacted according to the balanced chemical reaction: FeCl3(aq) + 3 AgNO3(aq) 6.022 × 1023 Oll 4 4.30 0.001 Question 31 of 34 169.88 FS % 5 143.32 1 6 → 0.500 3 AgCl(s) + Fe(NO3)3(aq) y 3 g AgCl LAgNO3 LAgCl MAGNO, mol AgCl mL AgNO3 OM MOO mL of 0.500 M AgNO3 is ANSWER 7 7 1.43 1000 U 60.0 8 RESET 2 12.9 1.70 mL AgCl Mar 2 5:27 delete ★ ✰ ☐ Submit + 0 backspace 180
Window Help ered: eq req Ereg Important values if needed... | b... M M 2req 2req 2req =2req M Visited MAY 11 S prod01-cnow-owl.cengagenow.com Submit Answer 85 According to the following reaction, how many moles of carbon dioxide will be formed upon the complete reaction of 32.0 grams of carbon monoxide with excess oxygen gas? 2CO(g) + O2(g) → 2CO2(g) mol carbon dioxide Retry Entire Group A 6 [Review Topics] [References] Use the References to access important values if needed for this question. Module 2 | OWLv2 MacBook Pro & 87 9 more group attempts remaining * CO € 8 A S OWLV2 | Online teaching and learning resource from C... N Previous Email Instructor Next Thu May 11 10:3 zoom □ + 0 Save and Exit + 11 bl 2 201 ngs