**The Vaporization of Methanol**The vaporization of methanol, represented by the equation:\[ \text{CH}_3\text{OH(l)} \rightleftharpoons \text{CH}_3\text{OH(g)} \]is an endothermic process, characterized by the following parameters:- **Enthalpy Change (\( \Delta H_{\text{vap}} \))**: 37.4 kJ/mol- **Entropy Change (\( \Delta S_{\text{vap}} \))**: 111 J/mol·KThe task is to calculate the boiling point of methanol (in °C) on a mountaintop, where the atmospheric pressure is 385 torr. It's assumed that \( \Delta H^\circ \) and \( \Delta S^\circ \) do not change appreciably with temperature.**Calculation Diagram Explanation**The image includes a diagram of a calculator displaying the calculation:- **Input**: Various numbers and operations are visible.- **Result**: A result of 52.96°C is shown, but it's crossed out, indicating a correction or reconsideration of the value.This illustration emphasizes the importance of careful calculations and re-evaluations in thermodynamic problem-solving. The vaporization of methanol \( \text{CH}_3\text{OH(l)} \rightleftharpoons \text{CH}_3\text{OH(g)} \) is an endothermic process in which \( \Delta H_{\text{vap}} = 37.4 \, \text{kJ/mol} \) and in which entropy increases, \( \Delta S_{\text{vap}} = 111 \, \text{J/mol} \cdot \text{K} \). Calculate the boiling point of methanol (in °C) on a mountaintop where the atmospheric pressure is 385 torr. (Assume \( \Delta H^{\circ} \) and \( \Delta S^{\circ} \) do not change appreciably with temperature).**Diagram Description:**On the right, there is an image of a digital calculator interface with numbers and basic operations. A calculation result is shown and crossed out with a red line, displaying "5181 °C". There are no additional graphs or diagrams in the image.

∆Hvap = 37.4KJ/mol ∆Svap = 111J mol-1K-1 Boiling Point at 385torr =? 385torr = 0.5065atm R = 8.314Jmol-1K-1 We know ∆Svap = ∆Hvap ÷ T 111J mol-1K-1 = 37400÷ Tb Tb = 336.93K This temperature is at 1atm pressure. We know Clausius Clapeyron equation:- ln(P1÷P2 ) = (∆Hvap ÷ R)((1÷ T2) - (1÷ T1)) ln(P1÷1 ) = (∆Hvap ÷ R)((1÷ T2) - (1÷ T1)) ln(0.5065 ÷ 1) = (37400 ÷ 8.314)((1÷336.93) - (1÷ T1) - 1.512 x 10-4 = (1÷336.93) - (1÷ T1) T1 = 320.959K T1 = 47.44oC

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Chemistry

The vaporization of methanol CH:OH(I) = CH3OH(g) is an endothermic process in which AHvap = 37.4 kJ/mol and in which entropy increases, ASvap = 111 J/mol·K. Calculate the boiling point of methanol (in °C) on a mountaintop where the atmospheric pressure is 385 torr. (Assume AH° and AS° do not change appreciably with temperature). 52,96 °C 1 2 3 6 C 7 8 9. +/- х 100 4.

The vaporization of methanol CH:OH(I) = CH3OH(g) is an endothermic process in which AHvap = 37.4 kJ/mol and in which entropy increases, ASvap = 111 J/mol·K. Calculate the boiling point of methanol (in °C) on a mountaintop where the atmospheric pressure is 385 torr. (Assume AH° and AS° do not change appreciably with temperature). 52,96 °C 1 2 3 6 C 7 8 9. +/- х 100 4.

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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