A major component of gasoline is octane (CH8). When octane is burned in air, it chemically reacts with oxygen gas (02) to produce carbon dioxide (C02 and water (H2O What mass of water is produced by the reaction of 8.2 of octane? gg Round your answer to 2 significant digits. x10 ? X Check Explanation Terms of 2019 McGraw-Hill Education. All Rights Reserved. MacBook Pro

A major component of gasoline is octane (CH8). When octane is burned in air, it chemically reacts with oxygen gas (02) to produce carbon dioxide (C02 and water (H2O What mass of water is produced by the reaction of 8.2 of octane? gg Round your answer to 2 significant digits. x10 ? X Check Explanation Terms of 2019 McGraw-Hill Education. All Rights Reserved. MacBook Pro

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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(CH₂(CH₂) CH₂) reacts with gaseous oxygen gas (0₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). Liquid octane What is the theoretical yield of water formed from the reaction of 43.4 g of octane and 277. g of oxygen gas? Be sure your answer has the correct number of significant digits in it. X
Gaseous butane CH3CH22CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . If 1.67g of carbon dioxide is produced from the reaction of 1.2g of butane and 7.6g of oxygen gas, calculate the percent yield of carbon dioxide. Be sure your answer has the correct number of significant digits in it.
(CONTINUED ON NEXT PAGE) 4. Let's say that the full volume of your flask is 325 ml. You heat the flask of air in a hot water bath at 89.0°C according to your thermometer. You then inverti into the cold water bath at 5.0°C Water enters the flask as the volume of the gas shrinks. a) Theoretically, what should the volume of the gas be after it sits in the cold water bath? b) You find that during your experiment that 65.0 mL of water has entered the flask. What is the experimental volume of the gas? c) What is your percent error for this measurement?
Report 2 decimal places for all your answers. Do NOT include units in your answer. BaCl₂ H₂O 208.23 Mass of anhydrous BaCl₂ (amu) Mass of H₂O molecules in Hydrate (amu) Mass of Hydrate (amu) Percent H₂O in Hydrate (%) O BaCl 208.23 0.00 At n 208.23 plete the table. 0.00 % 18.02 226.25 7.97% Select one: O a. BaCl, • H2O O b. BaClz • 2 H2O O c. BaCl2 • 3 H2O O d. The data is inconclusive: it could be either BaCl₂ H₂O OR BaCl₂.2 H₂O O e. The data is inconclusive: it could be either BaCl₂ 2 H₂O OR BaCl₂ 3 H₂O BaCl₂ 2 H₂O 208.23 51°F 36.04 244.27 14.8 0 % Compare the experimental percent water you calculated for the barium chloride hydrate in the Question 6 in this assignment (above) with the theoretical percent water values calculated from the possible formulas in the table above. Do you think that the formula for hydrate is BaCl₂ H₂O, BaCl₂ 2 H₂O, or BaCl₂3 H₂O? End BaCl₂ 3 H₂O 208.23 PgUp 54.06 262.29 20.6 40) % J 6 Manage 9:44 PM 10/9/2022 PgDn
olo 6 A major component of gasoline is octane (C,H,). When liquid octane is burned in air it reacts with oxygen (0,) gas to produce carbon dioxide gas and water vapor. Calculate the moles of water produced by the reaction of 1.1 mol of octane. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. OLX
Please do not round off intermediate calculations. Thank you.
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Wine goes bad soon after opening because the ethanol (CH₂CH₂OH) in it reacts with oxygen gas (O₂) from the air to form water (H₂O) and acetic acid (CH₂COOH), the main ingredient of vinegar. What mass of ethanol is consumed by the reaction of 1.30 g of oxygen gas? Be sure your answer has the correct number of significant digits. X G s
A chemist measures the amount of chlorine gas produced during an experiment. He finds that 224.g of chlorine gas is produced calculate the number of moles of chit gas produced round your answer to 3 significant digits
How many grams of oxygen are required to completely burn 5.90g of C3H8 in the following unbalanced equation? C3H8(g)+ O2(g)= CO2(g)+H2O(g)
Gaseous butane CH3CH22CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . If 34.3g of carbon dioxide is produced from the reaction of 29.06g of butane and 172.6g of oxygen gas, calculate the percent yield of carbon dioxide. Be sure your answer has the correct number of significant digits in it.
C3H3 + 502 3 CO, + 4 H20 2.30 moles of C3Hgare burned in a room with excess oxygen gas. How many moles of carbon dioxide are released into the atmosphere during this process? mol CO2 [Round your answer to the correct number of significant figures!]