The enthalpy of vaporization (AHvap) is determined from the Clausius-Clapeyronequation:In VP (-AHvap/R)(1/T) + C (Note: the form of this equation is linear: y = mx + b)Use a Google Sheets to calculate the values for the x and y axis from the data givenbelow and to plot the natural log of vapor pressure (In VP) versus the inversetemperature in Kelvin (1/T).Trial #T(K)VP(mmHg)1298.2 116.22301.1 138.73305.1 174.24308.4 205.715310.8 229.66313.3269.5Paste the data table into your spreadsheet so that Trial # is in cell A1.A new column is inserted on the spreadsheet between the T(K) and VP(mmHg) columnsfor the 1/T calculation.• What formula to calculate 1/T is typed into the cell directly to the right of 298.2(cell C2)?1/T

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A new column is inserted on the spreadsheet between the T(K) and VP(mmHg) columns for the 1/T calculation.

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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Question

The enthalpy of vaporization (AHvap) is determined from the Clausius-Clapeyron
equation:
In VP (-AHvap/R)(1/T) + C (Note: the form of this equation is linear: y = mx + b)
Use a Google Sheets to calculate the values for the x and y axis from the data given
below and to plot the natural log of vapor pressure (In VP) versus the inverse
temperature in Kelvin (1/T).
Trial #T(K)
VP(mmHg)
1
298.2 116.2
2
301.1 138.7
3
305.1 174.2
4
308.4 205.7
15
310.8 229.6
6
313.3
269.5
Paste the data table into your spreadsheet so that Trial # is in cell A1.
A new column is inserted on the spreadsheet between the T(K) and VP(mmHg) columns
for the 1/T calculation.
• What formula to calculate 1/T is typed into the cell directly to the right of 298.2
(cell C2)?
1/T

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Example #3) 15mL of 2.0M HCI is mixed with 30mL of 0.75M KOH HCI + KOH → H₂O + KCI AHreaction = Substance H₂O HC1 KC1 KOH AHreaction=AHproducts- AHreactants AHreaction = (AHH20+ AHKCI) - (AHHCI + AHKOH) AHreaction = (-286 + -419 - 1kg1 Let's calculate the limiting reagent to determine how many mols of water will be formed: Remember: Volume of reactant ÷ 1000 x Molarity of reactant x mole-to-mole ratio to water Here's the first reactant: 15mL of 2.0M HCI IS 1500 * 2.0 0.03 mol HCl 30 1000 Lof LOM KOH Let's do this for the second reactant, 30mL of 0.75M KOH 0.75 0.0225 mol KOH = -)-(-164 -61 mol H₂O) x AHf in kJ/mol -286 -164 -419 -480 The limiting reagent is the compound that produced the fewest number of moles. Multiply that number of moles buy the AH reaction that was calculated above kJ/mol = -/-3725 kJ - +_ - 480 10.0225 Calcu From here on out, you are on your own! Calculate the enthalpy of reaction, and then the limiting reagent. Next multiply the enthalpy of reaction by the…