Lab Data Volume sodium carbonate (ml) Molarity sodium carbonate (M) Volume calcium chloride (mL) Molarity calcium chloride (M) Observations The measurement became 200 Mass filter paper (g) Mass filter paper + precipitate (g) Calculated Observed mass calcium carbonate (g) Identify limiting reactant Expected mass calcium carbonate (g) Percent vield (%) 99.0 0.20 100.0 0.20 0.26 2.09 1.83 Sodium carbona 1 91 MY NOTES DI Water LAB DATA SHOW LABELS Wash/Waste 2.09 g TARE -

Lab Data Volume sodium carbonate (ml) Molarity sodium carbonate (M) Volume calcium chloride (mL) Molarity calcium chloride (M) Observations The measurement became 200 Mass filter paper (g) Mass filter paper + precipitate (g) Calculated Observed mass calcium carbonate (g) Identify limiting reactant Expected mass calcium carbonate (g) Percent vield (%) 99.0 0.20 100.0 0.20 0.26 2.09 1.83 Sodium carbona 1 91 MY NOTES DI Water LAB DATA SHOW LABELS Wash/Waste 2.09 g TARE -

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 160AE: You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of...

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The notation “(l)” after a substance’s formula indicates it exists in the __________ state.
You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation 2Na(s)+Cl22NaCl(s) After each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. Answer the following questions: a. Explain the shape of the graph. b. Calculate the mass of NaCl formed when 20.0 g of sodium is used. c. Calculate the mass of Cl2 in each container. d. Calculate the mass of NaCl formed when 50.0 g of sodium is used. e. Identify the leftover reactant, and determine its mass for parts b and d above.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
You have seven closed containers each with equal masses of chlorine gas (Cl2). You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chloride react to form sodium chloride according to the equation :math>2Na(s)+Cl2(g)2NaCl(s) ter each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. mg src=Images/HTML_99425-9-18ALQ_image001.jpg alt="" align="top"/> swer the following questions: l type='a'> Explain the shape of the graph. lculate the mass of NaClformed when 20.0 g of sodium is used.Calculate the mass of Cl2 , in each container. lculate the mass of NaClformed when 50.0 g of sodium is used. Identify the leftover reactant and determine its mass for parts b and d above.
For each of the following unbalanced reactions, suppose exactly 5.00 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. Na2B4O7(s) + H2SO4(o H3BOj(j) + Na2SO4(u CaC,(s) + H2O(/) Ca(OH)2(s) + C2H2(g) NaCl(s) + H2SO4(/> HCl(g) + Na2SO4(s) SiO2(s) + C(x) —> Si(/) + CO(g)
What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
A solution is 0.1% by mass calcium chloride. Therefore, 100. g of the solution contains g of calcium chloride.
g and lear X Your one-time code - escobedoa x G how do you cover a ml to liter -x + keAssignment/takeCovalentActivity.do?locator-assignment-take Use the References to access important values if needed for this question. According to the following reaction, how many moles of carbon dioxide will be formed upon the complete reaction of 31.9 grams of carbon (graphite) with excess oxygen gas? C(s) + O₂(g) → CO₂(g) mol carbon dioxide Submit Answer Q Search L Retry Entire Group Ws LPI 2 more group attempts remaining BAGNOdı hp ☆ 口 Previous OG 1 6:5 5/18/
Estimate Mass of oxalic acid 0.2237g dihydrate (g) Initial NaOH 0.11ml burette reading (ml) Final NaOH burette 34.52ml reading (ml) Observations overshot (i.e. light pink, dark pink, overshot) Volume of NaOH added (ml) Moles of oxalic acid dihydrate (mol) Mole ratio of NAOH to oxalic acid Moles of sodium hydroxide (mol) Molarity of NaOH, M
Mass Salicylic Acid used 0.1498 g Mass Acetic Anhydride used 0.3417 g Mass filter paper/funnel 7.8668g Mass filter paper/funnel/aspirin 28.7045g Mass aspirin synthesized 0.2295 g based on the data given above. what would the theoretical yield of aspirin be?
2911/15/-1 {J... macOS Monterey... Combining 0.287 mol Fe₂O3 with excess carbon produced 13.5 g Fe. Fe₂O3 + 3C 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: What is the theoretical yield of iron in moles? theoretical yield: Dashboard scyool What is the percent yield? percent yield: Resources mol mol %
X Macmilla X ck Course M X Submit Answer Sections X /index.html?deploymentid=5735112480241329813180832311&elSBN=9781305862883&id=1707786042&snapsh olchlometry of Reactions: Gram to Gram: This is group attempt 1 of 10 References HOMEWO X Use the References to access Important values if needed for this question. According to the following reaction, how many grams of potassium phosphate will be formed upon the complete reaction of 23.3 grams of phosphoric acid with excess potassium hydroxide ? potassium hydroxide(aq) + phosphoric acid(aq) →→→ potassium phosphate(aq) + water(1) grams potassium phosphate MindTap X Autosaved at 6:23 PM MacBook Air Gatoms to