Where did the last phase of H3O+ comefrom?Because quenching work is needed tomake it OH at the last stageIs it possible to do quenching work fromEt20?Please explain TT.TOCH3LIAIHA CI.2 eain)Et 20 (o.5M)1. o'c Smin2. R7 lominmethyl benzcateBenzyl alcoholLit-O LitO CH3AIH3O CH3H- Al -HLitAIH gHLitBenzl alcohol

Where did the last phase of H3O+ come from? Because quenching work is needed to make it OH at the last stage Is it possible to do quenching work from Et20? Please explain TT.T LIAIHA CI.2eain) Et 20 (o.5M) 1.0'c Smin 2. RT lomin OCH3 methyl benz0ate Benzyl alcohol O Lit AIH3 Lit O CH 3 O CH3 H- Al -H Lit Lit Benzyl alcohol

Where did the last phase of H3O+ come from? Because quenching work is needed to make it OH at the last stage Is it possible to do quenching work from Et20? Please explain TT.T LIAIHA CI.2eain) Et 20 (o.5M) 1.0'c Smin 2. RT lomin OCH3 methyl benz0ate Benzyl alcohol O Lit AIH3 Lit O CH 3 O CH3 H- Al -H Lit Lit Benzyl alcohol

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 9ALQ: At 1 atm, liquid water is heated above 100C. For this process, which of the following choices (iiv)...

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Over what temperature range are the reactions in Problem 40 spontaneous?
At 1 atm, liquid water is heated above 100C. For this process, which of the following choices (iiv) is correct for Ssurr? S? Suniv? Explain each answer. i. greater than zero ii. less than zero iii. equal to zero iv. cannot be determined
Which processes shown in this figure involve the phasetransition H2O(l )----->H2O(g)?
CompoundΔ?∘fΔ⁢Gf∘ (kJ/mol)A+387.7+387.7B+604.7+604.7C+402.0+402.0 Use the data given in the table to calculate the value of Δ?∘rxnΔ⁢Grxn∘ at 25∘25∘ C for the reaction described by the equation A+B↽−−⇀CA+B↽−−⇀C Δ?∘rxn=Δ⁢Grxn∘= If Δ?∘rxnΔ⁢Hrxn∘ and Δ?∘rxnΔ⁢Srxn∘ are both positive values, what drives the spontaneous reaction and in what direction at standard conditions? The spontaneous reaction is entropy-driven to the left. The spontaneous reaction is enthalpy-driven to the left. The spontaneous reaction is entropy-driven to the right. The spontaneous reaction is enthalpy-driven to the right.
Determine the Ecell and ΔG for the reaction of 2AgNO3 (aq, 1.0M) + Sn(s) ---> Sn(NO3)2(aq, 0.25M) + 2Ag(s) Ag+1(aq) + e- ---> Ag (s) E°= 0.80V Sn2+ + 2e- ---> Sn(s) E°= -0.14V
At 25oC, Ksp for copper(I) chloride (CuCl) is 1.0 x 10-6. Calculate ΔΔGo (kJ/mol) for the reaction: CuCl(s) ⇆ Cu+(aq) + Cl-(aq) Select one: a. 34.2 kJ/mol b. 3.42 x 104 kJ/mol c. -3.42 x 104 kJ/mol d. -34.2 kJ/mol
Use the data below to calculate ΔG°rxn for the reaction:A+2BC+DData:$$A+2B--->2CΔG°rxn = −235.0 kJ/molC--->D ΔG°rxn=200.0kJ/mol
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C(s, graphite) 0 0 5.69 CO(g) -110.5 -137.2 197.9 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 1. What is the value of ∆S⁰ for the oxidation of carbon to carbon monoxide, 2C(s, graphite) + O2(g) → 2CO(g) in J/K?
At 381 K, the following reaction takes place: Hg2Cl4(g) + Al2Cl6(g) --> 2 (HgAlCl5)(g) ΔH = +10 kJ (a) Offer an explanation for the very small ΔH for this reaction for the known structures of the compounds. (img 1) (b) Explain why the small ΔH in this reaction is evidence against (img 2) as the structure of Hg2Cl4(g).
18. Calculate the heat of reaction at constant volume for 5.00 g C3H8 ,considering the following chemical reaction: C3H8 (g) + O2(g) --------------------> CO2 (g) + H2O (g) heat of standard formation: O2 = 0.00 kJ / mole, H2O (g) = -245 kJ / mole, CO2 = -318 kJ/mole and C3H8 = -438 kJ / mole C3H8 = 44.09 g/mole Temperature is 33 oC a.412 kJb.-212 kJc.-789 kJd.-169 kJ
18. Calculate the heat of reaction at constant volume for 5.00 g C3H8 ,considering the following chemical reaction: C3H8 (g) + O2(g) --------------------> CO2 (g) + H2O (g) heat of standard formation: O2 = 0.00 kJ / mole, H2O (g) = -245 kJ / mole, CO2 = -318 kJ/mole and C3H8 = -438 kJ / mole C3H8 = 44.09 g/mole Temperature is 33 oC a. -789 kJ b. -212 kJ c. 412 kJ d. -169 kJ
If the plot of ln Ksp versus 1/T for a reaction yields a straight line with positive slope and positive y-intercept, what can be said about the spontaneity of the reaction?