Exercise 18.70Consider the evaporation of methanol at 25.0 °C:Part CCH3 ОН (1) — СH3ОН (9).Рсн,он — 110.0mmHgYou may want to reference (Page) Section 18.9 while completingthis problem.Express the free energy change in kilojoules to one decimal place.AG° =kJSubmitPrevious Answers Request AnswerX Incorrect; Try Again; 2 attempts remainingPart DPCH,OH = 13.00mmHgExpress the free energy change in kilojoules to one decimal place.HVα ΑΣφkJAG° =SubmitRequest AnswerPart E ?AG° =kJSubmitRequest AnswerPart EThe vapor pressure of methanol is 143 mmHg. Identify the best reason to explain why methanol spontaneously evaporates in open air at 25.0°C andstandard pressure (760 mmHg).O Under these nonstandard conditions, the partial pressure of methanol is lower than its vapor pressure.Heat can be added under these nonstandard conditions to increase the vapor pressure of methanol.O The calculated standard free energy change corresponds to a spontaneous reaction.O Calculations for a closed container show a partial pressure of methanol lower than its vapor pressure.SubmitRequest AnswerNext >Provide FeedbackMacBook Pro"8"8Th8Ams

ΔG∘(CH3OH(g))=-162.3 KJ.mol-1 ΔG∘((CH3OH(l))=-166.6 KJ.mol-1 ΔG∘ =ΔG∘(Products) -ΔG∘(Reactants) ΔG∘=-162.3 - (-166.6) = +4.3 KJPART C PCH3OH= 110.0 mmHg (GIVEN) ΔG=ΔG∘+R T lnQ ΔG∘=4.3 KJ/mol R=8.314 J/mol.K = 0.008314 KJ/mol.K T=298K Q=P(CH3OH) =110.0 mmHg ( 1mmHg =0.00133322 bar) =0.146655 bar ΔG∘=4.3 +0.008314* 298* ln(0.146655 ) = -0.456 KJ ΔG∘=-0.456 KJPART D PCH3OH= 13.00 mmHg (GIVEN) ΔG=ΔG∘+R T lnQ ΔG∘=4.3 KJ/mol R=8.314 J/mol.K = 0.008314 KJ/mol.K T=298K Q=P(CH3OH) =13.00 mmHg ( 1mmHg =0.00133322 bar) =0.0173319 bar ΔG∘=4.3 +0.008314* 298* ln(0.0173319 ) = -6.95 KJ ΔG∘=-6.95 KJ

Science

Chemistry

Consider the evaporation of methanol at 25.0°C: Part C CH3OH (1) + CH3 OH (9). Рсн,он — 110.0mmHg You may want to reference (Page) Section 18.9 while completing this problem. Express the free energy change in kilojoules to one decimal place. AG° = kJ

Consider the evaporation of methanol at 25.0°C: Part C CH3OH (1) + CH3 OH (9). Рсн,он — 110.0mmHg You may want to reference (Page) Section 18.9 while completing this problem. Express the free energy change in kilojoules to one decimal place. AG° = kJ

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

Calculate the ∆H°rxn for the reaction C(graphite) + 2H2(g) → CH4(g)from the following enthalpy changes: - Cgraphite + O2(g) → CO2(g) ∆H = -393.5 kJ - 2H2(g) + O2(g) → 2H2O(l) ∆H = -571.6 kJ - CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ∆H = -890.4 kJ
Use standard enthalpies of formation to calculate ΔH° for the following reaction: SnO2 (s) + 2 CO (g) → Sn (s) + 2 CO2 (g) The ΔHf° of SnO2 (s) is -907.5 kJ/mol. Be sure to enter a unit with your answer.
In the upper atmosphere, ozone is produced from oxygen gas in the following reaction. 3O2(g) → 2O3(g) Calculate ΔHo AND ΔSo for ozone formation. (Enter your answer in kJ and give 3 significant figures).
1.Consider the complete combustion of methane gas, CH4(g): Which of the following BEST describes the relationship between ΔH and ΔU? a.ΔH > ΔU b.ΔH = ΔU = 0 c.ΔH = ΔU d.ΔH < ΔU 2.Which of the following reactions would you expect to have the lowest ΔSo? a.CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) b.C2H4(g) + 2O2(g) → 2CO2(g) + 2H2O(g) c.C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(g) d.C2H6(g) + 7/2O2(g) → 2CO2(g) + 3H2O(g) 3.Which species would you expect to have the lowest standard entropy (So)? a.Cl2(g) b.I2(s) c.F2(g) d.Br2(l)
5. Calculate ΔH° for the reaction 2 C4H10 (g) + 13 O2 (g) → 10 H2O(g) + 8 CO2 (g) using the following information: (refer to image)
STANDARD MOLAR ENTHALPHY OR FORMATION AND REACTION: Calculate the ∆H° of the following reaction. (Use 3 decimal places for the value of ∆H°f and express your answer as well in 3 decimal places.)
Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 3.96 g of sucrose is combusted in a constant volume (bomb) calorimeter, 65.3 kJ of heat is liberated. Calculate ΔE for the combustion of 2.75g of sucrose. Calculate ΔH for the combustion of 2.75 g of sucrose.
Under what temperature conditions (low T, high T, all T, nonspontaneous at all T) would this reaction occur spontaneously? Explain your reasoning. 2NH4NO3(s) → 2N2(g) + 4H2O(l) + O2 (g) , ∆Horxn = -236.0 kJ
Given the data in the table below, determine ΔH°rxnfor the reaction 4NO (g) + 6 H2O (l) → 4NH3 (g) + 5 O2 (g)
The value of ΔE for a system that performs 190 kJ of work on its surroundings and gains 250 kJ of heat is in kj?
A 0.588 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.706 kJ °C-1. If the temperature inside the calorimeter increased from 25.0 °C to 29.9 °C, determine ΔrU for this reaction in kJ mol-1 (with respect to C5H12). Do not worry about how realistic the final answer is. Express answer in 2 significant figures.
Consider the following reaction: Sr(OH)2(s) → Sr2+(aq) + 2 OH-(aq) ΔHorxn = -19.3 kJ/ mol Sorxn = -218.3 J/ K mol Which of the following statements is true? Group of answer choices: - the reaction is always non-spontaneous - The reaction is nonspontaneous at all temperatures - The reaction is spontaneous only at high temperature - The reaction is spontaneous only at low temperature - ΔG < 0 and the reaction is always spontaneous