c) In an experiment to determine the molar mass of a volatile organic liquid, 0.46g of it was injected into a graduated gas syringe. On vapourisation, it occupied a volume of 240cm at 20°c and 760mmHg. i)How can you confirm that the liquid has been completely vapourised? ohon ii) Calculate the molar mass of the liquid

c) In an experiment to determine the molar mass of a volatile organic liquid, 0.46g of it was injected into a graduated gas syringe. On vapourisation, it occupied a volume of 240cm at 20°c and 760mmHg. i)How can you confirm that the liquid has been completely vapourised? ohon ii) Calculate the molar mass of the liquid

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

c) In an experiment to determine the molar mass of a volatile organic liquid, 0.46g of it was
injected into a graduated gas syringe. On vapourisation, it occupied a volume of 240cm at 20°c
and 760mmHg. on
DHow can you confirm that the liquid has been completely vapourised?
ii) Calculate the molar mass of the liquid

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Acetone has a vapour pressure of 53.3 kPa at 39.5 °C and 202.6 kPa at 78.6 °C. From the above data, obtain an equation to correlate the vapour pressure of acetone. (The equation should be in the form In(P)= -A/T + Co where P, is in kPa units. Find numerical values for A and Co) A= 5756 K, Co = 17.989 A= 4756 K, Co = 16.989 A= 3756 K, Co = 15.989 A= 2756 K, Co = 14.989
2) Draw the isobaric phase diagram at 1 atm of the following two-component liquid system: water (Boiling point = 100°C) and nitric acid (Boiling point = 86°C), with the mass percentage of nitric acid on the x-axis. When the liquid mixture contains 68 % nitric acid, an azeotrope with a boiling point of 120.5°C, is formed. Use the sketch to describe under which conditions pure nitric acid can be obtained by means of isobaric distillation.
The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressureof pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?
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Looking at the following image of a curve of partial pressures vs mole fractions of the two components A and B of an ideal mixture of liquids that obeys Raoult's Law where pa and pe are the partial pressures of the two liquids A and B respectively and xa and xg are the mole fractions of A and B respectively, which of the following statements is true? PA Pa R S A. The intercepts R and S are representative of the equilibrium vapour pressures of the components A and B respectively B. The intercepts R and S are representative of the equilibrium vapour pressures of the components B and A respectively C. The slopes of the two curves, red and blue, are representative of the equilibrium vapour pressures of the components A and B respectively D. Both (B) and (C) E. The slopes of the two curves, red and blue, are representative of the mole fractions of the components A and B respectively