None Question 8Glycine, NH2-CH2-COOH, is the simplest stable amino acid. Write an equation for the foreaction of glycine C2H5O2N from its constituent free elements in their most stable statestandard state conditions, so that the standard enthalpy of formation of glycine, AHO, issame as AHO of this reaction.rxnA. CH3COOH (1) + NH3 (g) → C2H5O2N (s) + H2 (g)B. CH3COOH (1) + N2 (g) + H2(g) → C2H5O₂N (s)C. 2 CO (g) + H2O (g) + NH3 (g) →C2H5O2N (s) + O2(g)D. 2 C (s) + H2(g) + O2(g) + ½ N2 (g) → C2H5O2N (s)E. 4 C (s) + 5 H2 (g) + 2 O2 (g) + N2 (g) 2 C2H5O2N (s)CBOEODA

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Answered: Question 8 Glycine, NH2-CH2-COOH, is…

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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powo 72 3. Calculate the heat of combustion (kJ) of propane, C3H8 using the listed standard enthalpy of reaction data: C3H8(g) + 5 O2(g) →3 CO2(g) + 4 H₂O(g) AH° = -103.8 kJ AH = -393.5 kJ AHO = -241.8 kJ 3 C(s) + 4 H₂(g) →→ C3H8(g) C(s) + O2(g) → CO2(g) H₂(g) + 1/2 O2(g) → H₂O(g) 4. Given the following equations and Ho values given below, determine the heat of reaction at 298 K for the reaction: 2 N₂(g) + 5 O₂(g) →2 N₂O5(g) AHO=-571.6 kJ AH°= -73.7 kJ AH°=-348.2 kJ (24 2 H₂(g) + O2(g) → 2 H₂O(1) N₂Os(g) + H₂O(1)→ 2 HNO3(1) N2(g) + 3 O2(g) + H₂(g) → 2 HNO3(1) HA
Calculate the enthalpy of combustion for kerosene. Assume that kerosene is C10H22(l) and that the products are CO2(g) and H2O(l). ΔH°f (C10H22(l)) = –249.6 kJ/mol ΔH°f (CO2(g)) = –393.5 kJ/mol ΔH°f (H2O(l)) = –285.8 kJ/mol Select one: a. –872.9 kJ/mol b. –5489.9 kJ/mol c. –429.7 kJ/mol d. –6829.2 kJ/mol
Which combination will give you the enthalpy change for the hydrogenation of ethene to ethane, AH3? ΔΗ ΔΗ, 20 (s) + 3H, (g) C,H, (g) + H¿ (g) C,H, (g) AH, ΔΗ + 20,(g) + 20, (g) 200, (g) + 3H, (g) -ΔΗ +ΔΗ-ΔΗ B. ΔΗ-ΔΗ+ ΔΗ C. ΔΗ + ΔΗ-ΔΗ D. -ΔΗ-ΔΗ+ ΔΗ А.
Acetylene burns in air according to the following equation: ΔΗ. AH СН (g) + O23) — 2 СО,(g) На0(g) =-1255.8 kJ rxn Given AH of CO2(g) =-393.5 kJ/mol and AH of H20(g)-241.8 kJ/mol, find AH of C2H2(g). f kJ/mol
Find the standard enthalpy of formation of ethyne gas, C2H2(g), given the following data: C2H2(g) + 5/2 O2(g) - 2 CO2(g) + H20(1) AH° = -1300 kJ C(s) + O2(g) – CO2(g) AH°; = -393.5 kJ H2(g) + 1/2 O2(g) - H20(1) AH°; = -285.8 kJ %3D O 227 kJ O -17 kJ 52 kJ 73 kJ 177 kJ
Q.29. Determine, at 298 K, Ar¡Hº, the standard enthalpy of the reaction (1) between hydroquinone with hydrogen peroxide to produce quinone. C,H4(OH)2(aq) + H2O2(aq) → CGH4O2(aq) + 2 H2O (E) (1) Knowing the standard reaction enthalpies, at 298 K, of the following reactions: (2) C6H4(OH)2 (aq) → C6H4O2 (aq) + H2 (g) ; A12H° = + 177.4 kJ mol-1 (3) H2 (g) + O2 (g) → H2O2 (aq) A:3H° = -191.2 kJ mol-1 (4) H2 (g) + ½0O2 (g) → H20 (g) A:4H° = -241.8 kJ mol-1 (5) H2O (g) H2O (€) ArsHº -43.8 kJ mol-1
b) Using the following data of heats of combustion in cal/g mole, calculate the following: (a) (b) Heat of vaporization of benzene – cal/g mole Heats of combustion of benzene to water i) C6H6 (1) → CO2 (g) and H2O (1) = 7,80,980 ii) C,H6 (g) → CO2 (g) and H2O (g) = 7,59,520 iii) H2 (g) → H2O (I) = 68,317 iv) H2 (g) → HO (g) = 59,798 v) Graphite to CO2 (g) = 94,052
[4] rxn 2. Given the following information, calculate AH for the reaction. 2C3Hs(g) +1002(g) → 6CO2(g) + 8H₂O(1) | AH¦ (C³H8(g)) = -103.9 kJ/mol; AH; (CO2(g)) = -393.5 kJ/mol, AH; (H₂O(1) = -285.5 kJ/mol
During the combustion of 5.00 gg of octane, C8H18C8H18, 239.5 kcalkcal (1002 kJkJ) is released. what is the balanced equation for the combustion reaction? How much energy (in kJkJ) is released by the combustion of 1.21 molmol of C8H18C8H18 ? How many moles of octane must be burned to release 442.4 kcalkcal ? How many kilocalories are released by the combustion of 18.3 gg of C8H18C8H18 ?
What is the standard enthalpy of isomerization (kJ/mol) of propanol to isopropanol in the liquid state?
(b) (i) Acetylene, C2H2 is a colourless gas which is widely used as a fuel and a chemical building block. Using the given enthalpies, calculate the standard enthalpy of formation of acetylene. AH°{CO2(g)] =-–393.5 kJ mol AH®[H2O(g)] = –285.8 kJ mol"1 AH°[C2H2(g)] =-1299.4 kJ mol"
From the enthalpies of the reaction H2(g)+F2(g)→2HF(g)AH=-537kJ C(s)+2F2(g) →CF4(g)AH=-680kJ 2C(s)+2H2(g) →C2H4(g)AH=+52.3kJ calculate AH for the reaction of ethylene with F2: C2H4(g)+6F2(g)→2CF4(g)+4HF(g)

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