1) Calculate the percent by volume of acetic acid by fermentation. Assumptions: No volumechanged during fermentation.Overall chemical reaction facilitated by Acetobacter aceti:C2H5OH+O2CH3COOHH206%Given: Volume of 6% C2H5OH = 3 LMolar mass of C2H5OH = 46.07 g/molMolar mass of CH3COOH = 60.06 g/molDensity of C2H5OH = 0.789 g/mLDensity of CH3COOH = 1.05 g/mLRequired: Percent acetic (% by volume) produced

Answered: Image /qna-images/answer/fa84f74b-eed2-4d1b-ad17-d5211779172d.jpg

Answered: 1) Calculate the percent by volume of…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 107QRT

See similar textbooks

Similar questions

1. 250.0 g each of toluene (CoHsCH:) and benzene (CsHs) are mixed together. Answer the following questions. C&H6 C6HSCH3 Compound M (g/mol) Kr (°C/m) | TP (°C) | Kb(C/m) 5.12 7.27 78.108 93.142 5.55 -95.0 2.53 3.29 To (°C) 81.1 110.7 (a) In this solution, which is the solute and which is the solvent? (b) What is the freezing point of this solution, in °C? (c) What is the boiling point of this solution, in °C? (d) Calculate the osmotic pressure of this solution in kPa. Assume that the masses are additive and the density of the final solution at 25°C is 0.867 g/mL.
Glycine is an amino acid made up of carbon, hydrogen, oxygen, and nitrogen atoms. Two samples of glycerine are combusted during an experiment to determine the empirical formula of glycerine. Sample 1: Combustion of a 0.2036 g sample produced 132.9 mL of CO2 at 25°C and 1.00 atm. and 0.122 g of water. Sample 2: 0.2500 g of glycine is treated in such a way that all the nitrogen atoms are converted to N2 gas. The volume of the nitrogen gas collected was 40.8 mL at 25°C and 1.00 atm. Determine: 1. The percentages of carbon and hydrogen in glycine. 2. The percentage of nitrogen in glycine. 3. The percentage of oxygen in glycine. 4. The empirical formula of glycine.
In the fermentation of sucrose to ethanol, Calculate how many milliliters of CO2 (at STP) would be produced if all the sucrose were fully oxidized by aerobic respiration. with 10g of sucrose.
If a student recrystallized 0.58g of impure acid and recovered 0.12 g of product, the percent recovery of the acid is: O 0.48% 20% 4.8% 0.2% f compound A (Mwt=46), with vapor pressure 400 mmHg at 5
C18H3602(s) + C5H14O4NP(s) + C3H8O3(aq) → 1.63 g Fatty Acid 3.2 mL of 0.98 M Choline Phosphate MW? 3.2 mL of 0.52 M Glycerol MW? g/mol MW? C44H88O8NP(s) + Theoretical g = ? Phospholipid MW = ? (a) Given the measured values, who is the limiting reactant for this equation? H₂O(1) Water 1.0 g/mL MW = ?
Wine goes bad soon after opening because the ethanol (CH3CH₂OH) in it reacts with oxygen gas (0₂) from the air to form water (H₂O) and acetic acid (CH₂COOH), the main ingredient of vinegar. What mass of water is produced by the reaction of 8.9 g of ethanol? Round your answer to 2 significant digits. 08 g x10 ? Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility Explanation Check X MacBook Pro & X
Experimental procedure. Be sure to wear gloves throughout this reaction. Place a magnetic stir bar, 2.0 g of trans- stilbene, and 40 mL of ethanol in a 125-mL Erlenmeyer flask. Note the shape and color of the crystals in your lab notebook. Clamp the flask in place on a magnetic stir/heat plate. With heating and stirring, dissolve the trans-stilbene. Be careful not to heat too quickly. Add 4.0 g of pyridinium tribromide. If solid material adheres to the interior walls of the flask, use a little ethanol to rinse it down. Heat with stirring for 5 minutes after the addition of reagents is complete. Remove the flask from the hot plate. Use caution to avoid getting burned by the hot flask. The product should quickly begin to precipitate or crystallize. Let the reaction mixture cool to room temperature. Chill the mixture in an ice bath. Collect the product by vacuum filtration in a pre-weighed fritted funnel or fritted crucible. Alternatively, use a ceramic Büchner funnel and filter paper. If…
Photosynthesis in plants converts carbon dioxide and water into glucose (C6H1206) and oxygen according to the equation below. 6CO2 (g) + 6H20a → C6H1206 (s) + 602 (g) Substance СО2 (8) H20M C6H1206 (s) 02 (g) kJ AH°; (mol -393.5 -285.8 -1273.3 J H° mol. k 213.6 69.9 209.2 205.0 Calculate the AHº, ASº, and AGº. Is the reaction spontaneous at standard conditions?
What is the mole ratio for O2 gas to water for the balanced equation for the complete combustion of butane. 2C4H10(g)+ 13O2(g)-> 10H2O(g) + 8CO2(g)
19) D CH₂CH3 HBC. ROOR 20) CH₂CH₂ CH₂C=C CH3 "H warm KMO/OH
Calculate the percent yield of ester for the esterification reaction of Isopentyl Acetate isopentyl alcohol- quantity: 3.177g acetic acid- quantity: 7mL isopentyl acetate (product)- 1.268g
Assuming that 50% of the heat is useful, how many kg of water at 15.0 oC can be heated to 95.0 oC by burning 200L of methane, CH4, measured at STP? Heat of combustion of methane is 211 kcalmol-1. Specific heat capacity of water is 1.00 kcal kg-1K-1.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

EBK A SMALL SCALE APPROACH TO ORGANIC L

Chemistry

ISBN:

9781305446021

Author:

Lampman

Publisher:

CENGAGE LEARNING - CONSIGNMENT

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

EBK A SMALL SCALE APPROACH TO ORGANIC L

Chemistry

ISBN:

9781305446021

Author:

Lampman

Publisher:

CENGAGE LEARNING - CONSIGNMENT

SEE MORE TEXTBOOKS