Wine is produced by the fermentation of grapes. In fermentation, the carbohydrate glucose (C6H₁206) is converted to ethanol (C₂H6O) and carbon dioxide (CO₂), according to the given balanced equation. CH₁₂O6(aq) 2C,H,O(aq) + 2 CO₂ (g) How many grams of ethanol (C₂H₂O) are formed from 0.75 mol of glucose (C6H₁206)? Be sure your answer has the correct number of significant figure g C₂H₂O 0x10 X Ś

Wine is produced by the fermentation of grapes. In fermentation, the carbohydrate glucose (C6H₁206) is converted to ethanol (C₂H6O) and carbon dioxide (CO₂), according to the given balanced equation. CH₁₂O6(aq) 2C,H,O(aq) + 2 CO₂ (g) How many grams of ethanol (C₂H₂O) are formed from 0.75 mol of glucose (C6H₁206)? Be sure your answer has the correct number of significant figure g C₂H₂O 0x10 X Ś

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

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 5.4 kgkg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)
Consider the combustion reaction of a hydrocarbon compound here: C2H4(g) + 302(g): 2 CO2(g) + 2 H20(g) ----> When 5.00 mol of C2H4 and 12.0 mol of O2 are added to the reactor, How many moles of CO2 can be produced by the reaction? O 4.00 mol of CO2 O 10.0 mol of CO2 O 5.00 mol of CO2 O 8.00 mol of CO2
If 200 kJ of heat are supplied, how many grams of NO can be produced? N2(g) + O2(g)→ 2 NO(g) AH = 180.6 kJ/mol O 66.5 g 54.2 g O 30.1 g O 2.21 g
When exposed to air, aluminum metal, AlAl, reacts with oxygen, O2O2, to produce a protective coating of aluminum oxide, Al2O3Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 a) What is the theoretical yield of aluminum oxide if 3.00 molmol of aluminum metal is exposed to 2.55 molmol of oxygen? Express your answer with the appropriate units.
Hydrogen gas reduces carbon dioxide gas to form methane (CH4) gas and steam. Choose the correct balanced net ionic equation (simplest whole-number coefficients) for this reaction.
The Apollo 13 mission astronauts are running out of oxygen and need to get rid of the excess carbon dioxide. You know that sodium hydroxide can remove carbon dioxide from the spacecraft cabin. The filter which they had been using is fully saturated and no longer works. The astronauts have a 5 kg container of sodium hydroxide on the ship. The reaction to neutralize the air, remove carbon dioxide with sodium hydroxide is shown below CO2(g) + 2NaOH(s) ⟶⟶ Na2CO3(aq) + H2O(l) The astronauts have 2 days left before they land on earth. You know that there are three astronauts, and each astronaut emits roughly 500. g of carbon dioxide each day. Is there enough sodium hydroxide in the cabin to cleanse the cabin air of the carbon dioxide, or are the astronauts doomed? Calculate how much sodium hydroxide is required to remove all the carbon dioxide from the three astronauts. Be sure to show all your work!
6. Consider the reaction: 4Al(s) + 3029) – > 2Al2O3(s) (a) If 9.00 moles of aluminum react with an excess of oxygen, how many moles of aluminum oxide are produced? (b) The production of 0.435 moles of aluminum oxide requires the reaction of moles of aluminum and (c) When 1.730 moles of aluminum reacts, moles of oxygen? moles of oxygen are consumed.
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH₂ (g) + 20₂(g) → HNO3(g) + H₂O (g) Suppose the yield of the first step is 61.% and the yield of the second step is 77.%. Calculate the mass of nitrogen required to make 10.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 Explanation Check. ☐ x10 8 X 09 0.0 S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |
Use the References to access important values if needed for this question. For the following reaction, 4.29 grams of oxygen gas are mixed with excess propane (C3Hg). The reaction yields 2.81 grams of carbon dioxide. (1) What is the theoretical yield of carbon dioxide? (2) What is the percent yield for this reaction? C3Hg (g) +50₂ (g) 3CO₂ (g) + 4H₂O(g) % grams
When H,S(g) reacts with O2(g) to form H,0(g) and SO2(g), 124 kcal of energy are evolved for each mole of H,S(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation.
15. Citric acid, C6H807 (aq), is often used as an additive to make candies "sour. a. Draw a flowchart that shows how to caloulate the molar mass of citric acid, b. Verify the steps in your flowchart by calculating the molar mass of citric acid.
Camels store the fat tristearin (C57H110O6) in their hump. As well as being a source of energy, the fat is a source of water, because of the following respiration reaction: 2 C57H110O6 (s) + 163 O2 (g) à 114 CO2 (g) + 110 H2O (l)What mass (g) of water can be made from 1.0 kg of fat?