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The mole fraction of Mgl2 of the solution in Part A is 1.59x10-2. Calculate the expected vapour pressure of the solution in Part A if the vapour pressure of pure water at 9.7 °C is 9.020 mmHg? 8.59 mmHg 9.16 mmHg O 8.88 mmHg O 7.73 mmHg O 0.431 mmHg

The mole fraction of Mgl2 of the solution in Part A is 1.59x10-2. Calculate the expected vapour pressure of the solution in Part A if the vapour pressure of pure water at 9.7 °C is 9.020 mmHg? 8.59 mmHg 9.16 mmHg O 8.88 mmHg O 7.73 mmHg O 0.431 mmHg

Chemistry
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
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The mole fraction of MgI2 of the solution in Part A is 1.59×10−2

The mole fraction of Mgl, of the solution in Part A is 1.59x10-2. Calculate the expected vapour pressure of the solution in Part A if the vapour pressure of pure water at 9.7 °C is 9.020 mmHg? 8.59 mmHg O 9.16 mmHg O 8.88 mmHg O 7.73 mmHg O 0.431 mmHg
Transcribed Image Text:The mole fraction of Mgl, of the solution in Part A is 1.59x10-2. Calculate the expected vapour pressure of the solution in Part A if the vapour pressure of pure water at 9.7 °C is 9.020 mmHg? 8.59 mmHg O 9.16 mmHg O 8.88 mmHg O 7.73 mmHg O 0.431 mmHg
A solution composed of 75.0 g magnesium iodide (Mgl2) in 300 g of water at 9.7 °C. What is the mole fraction of Mgl, in this solution? The molar mass of Mgl, is 278.1 g mol-1 and the molar mass of H20 is 18.02 g mol-1.
Transcribed Image Text:A solution composed of 75.0 g magnesium iodide (Mgl2) in 300 g of water at 9.7 °C. What is the mole fraction of Mgl, in this solution? The molar mass of Mgl, is 278.1 g mol-1 and the molar mass of H20 is 18.02 g mol-1.
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