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The mole fraction of iodine, I,, dissolved in dichloromethane, CH,CI,, is 0.115. What is the molal concentration, m, of iodine in this solution? First, assume that this solution with X= 0.115 has 1 mol CH,Cl,. Calculate the number of moles of I, if the moles of CH,CI, is 1. mol I, Now convert the 1 mole of CH,Cl, assumed in the previous section to mass in kg. kg CH,Cl, Now calculate the molality of the solution. m Reset this Activity Learning Dashboard Did I Get This Calculate the mole fraction of Cl, in a solution of 25.0 g of Cl, in 125 g of dichloromethane, CH,Cl,. Calculate the molality of the solution in the previous question. m Calculate the mole fraction of solute and solvent in a 0.750 m KNO, aqueous solution. XKNOS H2O

The mole fraction of iodine, I,, dissolved in dichloromethane, CH,CI,, is 0.115. What is the molal concentration, m, of iodine in this solution? First, assume that this solution with X= 0.115 has 1 mol CH,Cl,. Calculate the number of moles of I, if the moles of CH,CI, is 1. mol I, Now convert the 1 mole of CH,Cl, assumed in the previous section to mass in kg. kg CH,Cl, Now calculate the molality of the solution. m Reset this Activity Learning Dashboard Did I Get This Calculate the mole fraction of Cl, in a solution of 25.0 g of Cl, in 125 g of dichloromethane, CH,Cl,. Calculate the molality of the solution in the previous question. m Calculate the mole fraction of solute and solvent in a 0.750 m KNO, aqueous solution. XKNOS H2O

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
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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17) Calculate the mole fraction of solute and solvent in a 3.0 m solution of sodium chloride. Converting from one concentration unit to another is accomplished by first comparing the two unit definitions. In this case, both units have the same numerator (moles of solute) but different denominators. The provided molal concentration may be written as: 3.0molNaCl1.0kgH2O The numerator for this solution's mole fraction is, therefore, 3.0 mol NaCl. The denominator may be computed by deriving the molar amount of water corresponding to 1.0 kg 1.0kgH2O(1000g1kg)(molH2O18.02g)=55molH2O and then substituting these molar amounts into the definition for mole fraction. XH:0=molH2OmolINaC+molH:0XH:0=55molH:03.0molNaC+55molH:0XH:0=0.9 5 XNaCI=molNaClmolNaCl+molH20XNaC=3.0molNaC13.0molNaC+55molH20XNaC=0.05 2 Learn By Doing The mole fraction of iodine, I,, dissolved in dichloromethane, CH,Cl, is 0.115. What is the molal concentration, m, of iodine in this solution? First, assume that this solution with X= 0.115 has 1 mol CH,CI,. Calculate the number of moles of I, if the moles of CH,Cl, is 1. |mol I, Now convert the 1 mole of CH,CI, assumed in the previous section to mass in kg. kg CH,Cl, Now calculate the molality of the solution. т Reset this Activity Learning Dashboard Did I Get This Calculate the mole fraction of Cl, in a solution of 25.0 g of Cl, in 125 g of dichloromethane, CH,Cl,. Calculate the molality of the solution in the previous question. m Calculate the mole fraction of solute and solvent in a 0.750 m KNO, aqueous solution. XKN03 XH20
Transcribed Image Text:17) Calculate the mole fraction of solute and solvent in a 3.0 m solution of sodium chloride. Converting from one concentration unit to another is accomplished by first comparing the two unit definitions. In this case, both units have the same numerator (moles of solute) but different denominators. The provided molal concentration may be written as: 3.0molNaCl1.0kgH2O The numerator for this solution's mole fraction is, therefore, 3.0 mol NaCl. The denominator may be computed by deriving the molar amount of water corresponding to 1.0 kg 1.0kgH2O(1000g1kg)(molH2O18.02g)=55molH2O and then substituting these molar amounts into the definition for mole fraction. XH:0=molH2OmolINaC+molH:0XH:0=55molH:03.0molNaC+55molH:0XH:0=0.9 5 XNaCI=molNaClmolNaCl+molH20XNaC=3.0molNaC13.0molNaC+55molH20XNaC=0.05 2 Learn By Doing The mole fraction of iodine, I,, dissolved in dichloromethane, CH,Cl, is 0.115. What is the molal concentration, m, of iodine in this solution? First, assume that this solution with X= 0.115 has 1 mol CH,CI,. Calculate the number of moles of I, if the moles of CH,Cl, is 1. |mol I, Now convert the 1 mole of CH,CI, assumed in the previous section to mass in kg. kg CH,Cl, Now calculate the molality of the solution. т Reset this Activity Learning Dashboard Did I Get This Calculate the mole fraction of Cl, in a solution of 25.0 g of Cl, in 125 g of dichloromethane, CH,Cl,. Calculate the molality of the solution in the previous question. m Calculate the mole fraction of solute and solvent in a 0.750 m KNO, aqueous solution. XKN03 XH20
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The mole fraction of a compound in a solution is calculated by dividing the number of moles of a compound by the total number of moles present in the solution.

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