### Henry's Law and Vapor Pressure Measurements**Problem:**The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35 °C with the following results:| $ x_C $ | 0 | 0.20 | 0.40 | 0.60 | 0.80 | 1 ||------------|------|-------|-------|-------|-------|------|| $ P_C $ (torr) | 0 | 35.3 | 82.5 | 142 | 200 | 273 || $ P_A $ (torr) | 347 | 250 | 175 | 92.3 | 36.8 | 0 |The question asks for the Henry's law constant for chloroform in this system.**Options:**A) 365 torr B) 347 torr C) 177 torr D) 273 torr E) 485 torr **Solution:**Henry's law states that the vapor pressure of a solute (in this case, chloroform) is directly proportional to its mole fraction in the solution. Mathematically, it can be expressed as:\[ P_C = k_H \cdot x_C \]Where:- $ P_C $ is the vapor pressure of chloroform.- $ x_C $ is the mole fraction of chloroform.- $ k_H $ is the Henry's law constant.To find $ k_H $:We use any given pair of $ x_C $ and $ P_C $ values. For simplicity, let's use when $ x_C = 1 $:\[ P_C = k_H \cdot x_C \]\[ 273 \text{ torr} = k_H \cdot 1 \]\[ k_H = 273 \text{ torr} \]Therefore, the Henry's law constant for chloroform in this system is 273 torr.**Answer:**D) 273 torr

Given Data: xC00.20.40.60.81PC (torr)035.382.5142200273PA (torr)34725017592.336.80To…

The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35 °C with the following results: 0 0 347 A) 365 torr 0.20 35.3 250 0.40 82.5 175 XC Pc (torr) PA (torr) What is the Henry's law constant for chloroform in this system? 0.60 142 92.3 0.80 200 36.8 1 273 0

The vapor pressures of each component in a mixture of propanone (acetone, A) and trichloromethane (chloroform, C) were measured at 35 °C with the following results: 0 0 347 A) 365 torr 0.20 35.3 250 0.40 82.5 175 XC Pc (torr) PA (torr) What is the Henry's law constant for chloroform in this system? 0.60 142 92.3 0.80 200 36.8 1 273 0

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

grammarly-G X * Content oard.odu.edu/ultra/courses/_393452_1/cl/outline F2 Question Completion Status: X GA student wan X 1 QUESTION 3 A student wants to determine the solubility of water and copper (1) bromide (a green solid) in ethyl acetate (a colorless organic liquid). She places 1 mL of ethyl acetate into each of two test tubes. To one, she adds 5 drops of water to it. To the other, she adds a small scoop of copper(1) bromide. 8.0 F3 2 - Which test tube represents the ethyl acetate and A. Test tube 1 copper(1) bromide if the copper(1) bromide is insoluble in ethyl B. Test tube 2 acetate? C. Test tube 3 D. Test tube 4 - Which test tube represents the mixture of the ethyl acetate and water if the water is insoluble in ethyl acetate? $ Question Com X C Chegg Search x 3 Which test tube represents the mixture of the ethyl acetate and water if the water is soluble in ethyl acetate? - Which test tube represents the ethyl acetate and copper(1) bromide if the copper(1) bromide is soluble…
Consider the Solubility Curve for this Problem: Analysis for KClO3 & NH4Cl MW (KClO3) = 122.55 g/mol , MW (NH4Cl) = 53.49 g/mol i) What is the temperature at which KClO3 & NH4Cl both have the same solubility? Round to nearest degree. +/- 1° T = °C ii) What is the solubility (g per 100g H2O) at this temperature. Round to nearest gram. +/- 1 g s (KClO3) = g/100g H2O s (NH4Cl) = g/100g H2O iii) What is the molar solubility for KClO3 at this temperature? Assume the density of the solution is 1.21 g/cc. Round off to 2 sig. figs. |s| KClO3 = M iv) Calculate the Ksp for each of these chemicals at this temperature. Ksp = v) What is the unit of Ksp for KClO3? Unit for Ksp =
The literature value of the Ksp for calcium iodate is 6.47 × 10–6 at 25 °C. Use the following equation to calculate the percent error in your determination of the solubility product for calcium iodate. Note: Do not be alarmed if your average deviation is very large. This is not uncommon in Ksp experiments, even under the most careful conditions. Percent error = (|experimental value - literature value|)/ (literature value) X 100%
At a certain temperature, the solubility of zinc(I) chromate is (7.6x10^-5) M. What is the Ksp? Report your answer to 2 sig figs. Note: Your answer is assumed to be reduced to the highest power possible
Please answer this question as fast as you can please and tahnk you. I will afterwards write an wonderful review on solving the question. Thank you. Why is it important for us to leave the water for 5 minutes and determine the water's temperature? The density of water will vary with temperature. You want the water to equilibrate to room temperature in order to maintain consistent results. You want to wait so that the dissolved solids in the water settle to the bottom of the flask. It is impossible to determine the density of water below 20 °C with plastic beakers and cylinders so you need to wait for the water to warm up. It's not that important, we just want to stretch out the time of the experiment.
Inorganic Chem Please help answering this question Use equation V = (N)(q1)(q2)(k) / r where k = 9.0x10^9
O e) % KBr = % 66.2 , % KCI = % 33.8 %3D The solubility product (Ksp) for 4 points Pb(OH)2 (s) is 2.5 x 10-16. What would be the quantity of solubility by g/L of Pb(OH)2 which has Mwt =241.2 g/mole)? O 9.947 x 10-4 O 5.975 x 10-4 O 7.596 x 10-5 O 9.575 x 10-4 O 9.723 x 10-4 Calculate [H+], PH and POH 4 points
› Calculate the value of the equilibrium constant, Kỵ, for the reaction Q(g) + X(g) — 2M(g) + N(g) given that Kc = M(g) — Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.48 Kc2 Kc3 = 0.587 = = 13.6
Using the Kf and Kb equations with electrolytes A certain liquid X has a normal boiling point of 110.90 °C and a boiling point elevation constant K=1.66 °C-kg mol -1 .A solution is prepared by dissolving some ammonium sulfate ((NH SO,) in 150.g of X. This solution boils at 112.2 °C. Calculate the mass of (NH), SO, that was dissolved. Round your answer to 2 significant digits. ? Explanation Check ©2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | étv A
In lecture I mentioned that standard state is usually at 25oC; however, it can be at any specified temperature. In problems 9 and 10 you will calculate ΔGo from Ksp data. The Ksp range over the temperature range in these two problems is consistent with some actual solubility data; however, in order to allow each student to do their own calculation I have made this data for an "unknown" ionic solid. Calculate the value of ΔGo (kJ/mol) at 3.3oC for the dissolution of an ionic solid with a Ksp of 2.5 x 10-11 at 3.3oC. Your answer should have 2 sig figs.
The following data were collected for the reaction 2A + 2B + C 3G+ 4 F Experiment 2 3 4 5 [A] Units of Molarity .00125 .00250 .00125 .00125 .00301 [B] Units of Molarity 00125 .00125 00302 00302 .00100 [C] Units of Molarity 00125 .00125 .00125 00375 .00115 Rate Units M/s 00870 .0174 .0508 .457 a. What is the order with respect to each reactant and what is the overall order for the reaction? Answer this question within the answer box and show your work clearly labeled on the scratch paper. b. Write the rate law for the reaction. Answer this question within the answer box and show your work clearly labeled on the scratch paper. c. What is the value and units for k? Answer this question within the answer box and show your work clearly labeled on the scratch paper. d. Predict the rate for experiment 5, you should give a value and units. Answer this question in the answer box and show your work on the scratch paper labeled clearly.
Calculate the solubility of Fe(OH), in water at 25 °C. You'll find K.n data in the ALEKS Data tab. 2 sp Round your answer to 2 significant digits. g |x10 L ?