From your data in Part 1 of the experiment, you calculate the natural log of the partial pressure of water and 1/T value in K for 5 points between 50°C and 80°C. You make a graph of In(P) vs. 1/T and determine that the slope of the linear line is -4800 K. Use this information to calculate AHvap of water. Make sure to use R = 8.314 J mol-1 K-1. Oa. 46.6 kJ/mol Ob. 0.578 kJ/mol Oc. 31.5 kJ/mol O d. 39.9 kJ/mol

From your data in Part 1 of the experiment, you calculate the natural log of the partial pressure of water and 1/T value in K for 5 points between 50°C and 80°C. You make a graph of In(P) vs. 1/T and determine that the slope of the linear line is -4800 K. Use this information to calculate AHvap of water. Make sure to use R = 8.314 J mol-1 K-1. Oa. 46.6 kJ/mol Ob. 0.578 kJ/mol Oc. 31.5 kJ/mol O d. 39.9 kJ/mol

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

A certain substance X condenses at a temperature of 128.4 °C. But if a 800. g sample of X is prepared with 81.06 g of urea ((NH,), CO) dissolved in it, the sample is found to have a condensation point of 129.7 °C instead. Calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. -1 | °C mol Submit Assignment O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center EPIC MacBook Pro esc ZAA & #3 delete 8. R. ock W alt command command option
Only typed solution.
C2.
The vapor pressure of water at 30 °C is 4.24 kPa. Calculate the vapor pressure if 65.0 g of glycerol, C.H.O.(1), is added to 100.0 mL of water. The density of water at 30 °C is 0.996 g.mL-¹.
In this lab, you will determine the vapour pressure (P) of water at various temperatures and use this data to find its enthalpy of vaporization (AvapH). More generally, for an unknown liquid: if a plot of In P vs. 1/T gives a slope of -8038 K, what is its AvapH in kl/mol? Do not worry about how realistic the value is. Assume R = 8.314 J mol- K-.
Determine the molar mass of an unknown compound if the solution formed when 3.28 g of the compound dissolves in 100.0 g of benzene boils at 80.9C. Is the answer 108g? I used 80.1 as normal boiling point and 2.64 as Kb.
Number 2
10.The diagram below is an example of Liquid-Solid-Temperature Composition Phase Diagram of Completely Immiscible Solids. The left vertical line is B rich while the right vertical line is A-rich.Define the phases present in the region from A to E. |LS – TZ Phase Diagram: Completely Immiscible Solids This LS- TZ phase diagram is for completely immiscible solids. XA = 0 X = 1 XA = 1 X = 0 T =T?, At the solid phase, the system consists of 2 distinct solids A and B. T= T At the liquid phase, the system is called a melt. At the 2- phase regions, the system consists of either pure solid A or B and the melt. The composition of A in the melt can be traced along the liquidous curve. T T= Teu E At the solidous line, the system consists of solids A, B, and melt in which the composition of A, or y =1 Z, can be determined. Ya = 0 Zeut,a Za YA =1 Yn = 0 At the eutectic composition, minimum temperature is required to melt the mixture.
* 00 LL LI #3 The normal freezing point of a certain liquid X is -2.70 °C, but when 43.3 g of potassium bromide (KBr) are dissolved in 400. g of X the solution freezes at -9.6 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Round your answer to 2 significant digits. °C-kg K. mol Check Save For Later Submit Assignme O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibil MacBook Pro 114 F8 F3 F4 $4 3. 5. 6. P. A G H. K. B alt alt option command command option
The molar mass of liquid A = 85.0 g / mole, that of B = 112.0 g / mole. At 100 C, a solution of mass percentage in A equal to 30.0%, considered ideal, has a vapor pressureof equilibrium equal to 110 kPa. The vapor in equilibrium with this solution has a mole fraction of A equal to 0.450.A) Determine the equilibrium vapor pressure of pure A and that of pure B at 100 oCb) Determine the mass of A which must be added to 100 g of B to obtain a solution whosenormal boiling point is 100 C.
Some water dissolves in liquid methane at -161°C to givea solution in which the mole fraction of water is 6.0 × 10-5. Determine the mass of water dissolved in 1.00 L ofthis solution if the density of the solution is 0.78 g cm-3.
In this lab, you will determine the vapour pressure (P) of water at various temperatures and use this data to find its enthalpy of vaporization (AvapH). More generally, for an unknown liquid: if a plot of in P vs. 1/T gives a slope of -5949 K, what is its AvapH in kl/mol? Do not worry about how realistic the value is. Assume R = 8.314 J mol-¹ K-¹ Answer: