Homework 4 - Weeks 8 & 9 - Formulas and States8/18 tasks attempCitric acid (CeH;O7), named for its natural occurrence in citrus fruits, is produced in large quantitiesindustrially. This is often achieved through large-scale fermentation of sucrose and/or glucose. The reactioninvolving sucrose is summarized below:C12 H22O11 +3 O22 C6H3O7 +3 H2OHow many grams of citric acid would be produced from 900.0 kg of sucrose assuming a percent yield of87.10 % ?MassHelpful tip: To enter a number in scientific notation, enter 1.0E5 or 1.0e5, for 1.0 x 105 where the E# (or e#) denotes 10SAVE RESPONSE9.101118Book ProSearch or tyne URI

% yield = ( actual mass/ theoretical mass )×100

8/18 tasks attemp Citric acid (Ce H,O-) , named for its natural occurrence in citrus fruits, is produced in large quantities industrially. This is often achieved through large-scale fermentation of sucrose and/or glucose. The reaction involving sucrose is summarized below: C12 H22O1+302 2 C,HgO7 +3 H20 How many grams of citric acid would be produced from 900.0 kg of sucrose assuming a percent yield of 87.10 % ? Mass Helpful tip: To enter a number in scientific notation, enter 1.0E5 or 1.0e5, for 1.0 x 105 where the E# (or e#) denotes 10 SAVE RESPONSE

8/18 tasks attemp Citric acid (Ce H,O-) , named for its natural occurrence in citrus fruits, is produced in large quantities industrially. This is often achieved through large-scale fermentation of sucrose and/or glucose. The reaction involving sucrose is summarized below: C12 H22O1+302 2 C,HgO7 +3 H20 How many grams of citric acid would be produced from 900.0 kg of sucrose assuming a percent yield of 87.10 % ? Mass Helpful tip: To enter a number in scientific notation, enter 1.0E5 or 1.0e5, for 1.0 x 105 where the E# (or e#) denotes 10 SAVE RESPONSE

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 75QRT

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Classify each of the reactions according to one of the four reaction types summarized in Table 18.1. (a) C6H12O6(s) + 6 O2(g) 6 CO2(g) + 6 H2O() rH = 673 kj/mol-rxn rS = 60.4 j/K mol-rxn (b) MgO(s) + C(graphite) Mg(s) + CO(g) rH = 490.7 kJ/mol-rxn rS = 197.9 J/K mol-rxn TABLE 18.1 Predicting Whether a Reaction Will Be Spontaneous Under Standard Conditions
Identify each chemical reaction as synthesis, decomposition, single-displacement, double displacement, or combustion. 1) 2SO2 + O2 --> 2SO3 2) Al2(SO4)3 + 3Ca(OH)2 --> 2Al(OH)3 + 3CaSO4 3) 2C2H2 + 5O2 --> 4CO2 + 2H2O 4) Mg + 2AgNO3 --> Mg(NO3)2 + 2Ag 5) 3Ba(NO3)2 + 2H3PO4 --> Ba3(PO4)2 + 6HNO3 6) Mg(ClO3)2 --> MgCl2 + 3O2 7) 2Be + O2 --> 2BeO 8) 2Al + 3CuSO4 --> Al2(SO4)3 + 3Cu 9) 2PbO2 --> 2PbO + O2 10) 2C2H6 + 7O2 --> 4CO2 + 6H2O
se: C x O Edward V x O procedur x G traductor x E Imt rgt ch x O Course H X O Part The x C Part A A x /course.html?courseld=17244391&0penVellumHMAC=Dad27de605f424ee63856c9b0420083fd#10001 Part C The balanced reaction for the combustion of ethane is shown in the table, You allow 2,4 mol of ethane (C2H6) to react with 3.5 mol oxygen (O2). Complete the following ICF table, which may be done using the Simulation, to indicate the amounts of all chemical species for the initial, change, and final conditions. Drag the appropriate amounts to their respective targets. > View Available Hint(s) Reset Help 14 mol 7.2 mol 0.0 mol 8.4 mol 4.8 mol 1.0 mol 24 mol 2.0 mol 3.0 mol 3.5 mol 2C,H(g) + 7O2(g) → 4CO2(g) + 6H20(g) Initial Change Final P Pearson Copyright © 2022 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy I Permissions I Contact Us | O VI 10:37 DII backs & %23 %$4 % 7 4. 5 u r t y e
balance the chemical equation for each reaction C2H2Cl4 + Ca(OH)2-----> C2HCl3 + CaCl2 + H20
8 Reactions between certain organic (alkyl) halides and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane). (CH3)3CBr(aq) + H2O(1) →(CH3)3COH(aq) + H*(aq) + Br "(ag) k[(CH3)3CB1]. The accepted mechanism for the The experimental rate law is rate = %3D reaction is shown below. (1) (CH3)3C-Br(aq) →(CH3)3C*(aq) + Br "(aq) [slow] (2) (CH3)3C*(aq) + H2O(1) →(CH3)3C-OH2*(aq) [fast] (3) (CH3)3C-OH2*(aq) →H*(aq) + (CH3)3C-OH(aq) [fast] a) Why doesn't H2O appear in the rate law? b) Write rate laws for the elementary steps. c) What intermediates appear in the mechanism? d) Show that the mechanism is consistent with the experimental rate law. ed to the of consumption of N
For each of the following reactions, indicate if there is something wrong with the reaction. If something is wrong, say what it is.a) 2H2(g) + O2(g) 2H2O(l)b) C(s) + H2O(p) CO(g) + H2(g)c) N2(g) + H2(g) NH3(g)d) Cℓ2O7() + H2O(l) 2HBrO4(aq)
In the oxidation of carbon monoxide to carbon dioxide, 2CO(g) + O₂(g) - 2CO₂(g)
18 # 3 [Review Topics] [References] Use the References to access important values if needed for this question. When CO(g) reacts with O₂(g) to form CO₂(g), 67.6 kcal of energy are evolved for each mole of CO(g) that reacts. Write a balanced equation for the reaction with an energy term in kcal as part of the equation. Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not needed, leave it blank. 20 F3 E D Submit Answer C $ 4 288 R F % 5 V Retry Entire Group 7 more group attempts remaining FG ♫ tv IA O T G + 6 B MacBook Air F6 Y H & 7 N F7 - U J * 8 M DII FB 1 ( 9 K DD F9 O + V- ) 0 L A F10 command P 3 3 I O A ; option Email Instructor P11 { [ Previous ? + = 11 1 Next Save and Exit F12 delete BI return shift
O2 consumed by an individual (CO2 exhaled in liters)/(O2 inhaled in liters). It is used as a measure of basal metabolic rate and can indicate which types of molecules are being used by a person to produce energy. For glucose (C6H12O6), this value is 1 as the equation for the complete oxidation of glucose is: C6H12O6 + 6 O2 → 6 CO2 + 6 H2O If 4 of the CO2 molecules are produced by the citric acid cycle, which pathway or enzyme step is likely responsible for the production of the other 2 CO2 molecules produced during the complete oxidation of glucose by metabolism? a) Gluconeogenesis b) Glycolysis c) Beta Oxidation d) Urea Cycle
OH H2SO4 (catalyst) + 2 CH3CO₂H
IRS whistleblowers testify at Hou: XM $4 off on Delicious, Rejuvenating X A ALEKS-Andrew Herrera - Learn X ← → C www-awa.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-lvgXwPgmUhvlTCeeBZbufuBYTi0Hz7m7D3ZcZsVtNxxGh3NolGhgexjUoyas3VCHOBjufyala7Wgbxc... ☆ = @ 89°F Near record Fill in the information missing from this table: 4- ELECTRONIC STRUCTURE AND CHEMICAL BONDING Calculating the capacity of electron subshells subshell 3s 5s Explanation 4p 2 Some electron subshells principal quantum number n 0 0 0 Check }° с angular momentum quantum number / ▬▬ 0 0 0 Q Search FO maximum number of electrons 0 П 10 F7 F8 8 F9 X 3 en F10 *- OF ** PrtSc W 0/3 Insert © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility @dx a Delete Andrew ^ 0 olo Ar O X ⠀ 4:45 PM 7/20/2023
4. Sucrose is a disaccharide made up of glucose and fructose. Honey is a mixture of glucose and fructose. Explain why honey is a quicker source of energy than sucrose. Include a chemical reaction in your explanation. CH-OHbo 1oodOM 10 coitaforv &ar bon antndos ruol sleriadow ioiur edio insmazat ai oi ora oTiliw orido boteorlo vel bouch rus f td CHOH HO OF CH;OH OH OH Sucrose 5. Condensation reactions (also known as dehydration synthesis) are a very common type of organic reaction. Describe what happens in a condensation reaction and give two different examples of condensation reactions involving carbohydrates, lipids, or amino acids (each example should involve different types of compounds, ex: one example using carbohydrates and another example using lipids.) Indicate what types of compounds are involved in each example. HO 12. Bev show 6. Hydrolysis reactions are a very common type of organic reaction. Describe what happens in a hydrolysis reaction and give two different examples of…