The molar mass of the dissolved solute and molecular formula for it should be calculated. Concept introduction: The properties which depend on the number of moles of solute irrespective of its nature are termed as colligative properties. Relative lowering in vapor pressure, depression in freezing point, and osmotic pressure are examples of colligative properties.

Question

When 14.3 g of a certain molecular compound X are dissolved in 85.0 g of benzene C6H6, the freezing point of the solution is measured to be 0.5 °C. Calculate the molar mass of X. molal freezing point depression constant (Kf)°C·kg·mol−1 of benzen is 5.07 If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.

Answer 1

Question

Chapter 11, Problem 76AP

Interpretation Introduction

Interpretation:The molar mass of the dissolved solute and molecular formula for it should be calculated.

Concept introduction:The properties which depend on the number of moles of solute irrespective of its nature are termed as colligative properties. Relative lowering in vapor pressure, depression in freezing point, and osmotic pressure are examples of colligative properties.

Expert Solution & Answer

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Students have asked these similar questions

When 14.3 g of a certain molecular compound X are dissolved in 85.0 g of benzene C6H6, the freezing point of the solution is measured to be 0.5 °C. Calculate the molar mass of X. molal freezing point depression constant (Kf)°C·kg·mol−1 of benzen is 5.07 If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.

Calculate the value of the equilibrium constant, Ke , for the reaction Q(g)+X(g) = 2 M(g)+N(g) given that M(g) = Z(g) 6 R(g) = 2 N(g) + 4 Z(g) Kel 3.65 Kc2 = 0.420 3 X(g) + 3 Q(g) 9R(g) Kc3 13.4 K.

What mass of a non-electrolyte solute is required, when mixed with 225 g H2O, to change the equilibrium vapor pressure of H2O from 1.013 x 105 Pa to 8.104 x104 Pa, at approximately 110 °C? The molar mass of the non-electrolyte solute is 62.07 g mol−1. Assume ideal behaviour for the solution.