A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of80.0 mm Hg) and ChemicalB (with a pure vapor pressure of 100.0 mm Hg). Thesolution has a total vapor pressure of (9.66x10^1) mm Hg.If the solution is known to be made from 3.00 mol of A, how many moles of B mustthere be in the solution?HINT: The total pressure is the sum of each chemical's partial pressure: Pt = PA +PB.Use PA = XA PA° for both the partial pressure of chemicals A and B.Enter your answer in scientific notation with 3 sig figs. Do not include any units inyour answer.Do not round any intermediate calculations.Note: Your answer is assumed to be reduced to the highest power possible. A certain pure solvent freezes at 39.8°C and has a freezing point depressionconstant Kf = 0.777°C/m. What is the predicted freezing point (in °C) of a solutionmade from this solvent that is (1.46x10^0) m in a non-electrolyte solute?Enter your answer in scientific notation with 3 sig figs. Do not include any units inyour answer.Do not round any intermediate calculations.Note: Your answer is assumed to be reduced to the highest power possible.

Given data,Q1) Pure vapor pressure of chemical A=80mmHgPure vapor pressure of chemical…

A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and Chemical B (with a pure vapor pressure of 100.0 mm Hg). The solution has a total vapor pressure of (9.66x10^1) mm Hg. If the solution is known to be made from 3.00 mol of A, how many moles of B must there be in the solution?

A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and Chemical B (with a pure vapor pressure of 100.0 mm Hg). The solution has a total vapor pressure of (9.66x10^1) mm Hg. If the solution is known to be made from 3.00 mol of A, how many moles of B must there be in the solution?

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

A solution of KCl in water has Xkcl= .0700. What is the molality?
A solution of hexane, C6H14, in benzene, C6H6, has a molality of 0.250 m. What mass of hexane is dissolved in 400 g of benzene in this solution? mass C6H14 = [?] g mass Hexane (g) Enter
A solution is prepared by dissolving 5.88 g of an unknown nonelectrolyte in enough water to make 0.355 L of solution. The osmotic pressure of the solution is 1.21 atm at 27.0 °C. What is the molar mass of the solute?(R = 0.08206 L⋅atm/mol⋅K)
A solution contains 0.154 mol NaCl and 0.957 mol H, 0. Calculate the vapor pressure of the solution at 55 C. The vapor pressure of pure water at 55 °C is 118.1 torr. (Assume that the solute completely dissociates.) Express your answer with the appropriate units. P(solution) = 99.09 torr
Calculate the molality of a solution formed by adding 3.159 g of methanol (CH3OH) to 100.00 mL of water. The density of water is 0.9982 g/mL. DO not include units. The lattice energy for KF is 821 kJ/mol. The enthalpy of hydration for K+ is -336 kJ/mol and the enthalpy of hydration for F- is -431 kJ/mol. What is the enthalpy in kJ when 14.91 g of KF forms an aqueous solution? (Hint: start by finding the enthalpy of solution)
A) Calculate the Molarity5.35 g Mn(NO3)2 * 2H2O in 175 mL of solutionB)What is the molality of a solution formed by dissolving 1.00 mol of KCl in 16.0 mol of water?Express the concentration in moles per kilogram to three significant figures.C)How many grams of sulfur (S8) must be dissolved in 100.0 g naphthalene (C10H8) to make a 0.13 m solution?Express the mass in grams to two significant figures.
The boiling point of pure chloroform is 61.20°C.,A solution of 100.0 g of chloroform and 2.67 g of azulene, C10H8, has a boiling point of 61.70 °C. A solution of 100.12 g of chloroform and 1.00 g of the newly discovered compound torontonoate has a boiling point of 62.60 °C. What is the molar mass of torontonoate? Report your answer to one decimal place. Do not enter units.
[Item #3] *refer to the photo below*
Your pure water boils at 100.00 C. You add some sugar into it and now it boils at 101.20C. What is the molality? Kb= 0.512 Ckg/mol
Ex7; An aqueous solution of sodium hydroxide contains 20.0% NaOH by mass. It is desired to produce an 8.0% NaOH solution by diluting a stream of the 20% solution with a stream of pure water. Calculate the ratios (liters H20/kg feed solution) and (kg product solution/kg feed solution). F =? kg = 0.2 XNaOH P =? kg XH,0 = 0.8 F2 =? kg F2 = 0.08 kg Na0H/kg xH,0 = 0.92 kg H20/kg %3D 1
A solution of H2SO4(aq) with a molal concentration of 2.24 ? has a density of 1.135 g/mL. What is the molar concentration of this solution?
A chemist wants to determine the molar mass of a naturally occurring substance isolated from spearmint. She adds 5.131 g of this substance to 25.00 g of acetone (C3H6O; molar mass 58.08 g/mol). The vapor pressure of the solution is determined to be 0.2444 atm at 25°C. If the vapor pressure of pure acetone at this temperature is 0.2630 atm, what is the mole fraction of the solvent in this solution? Give your answer to four significant digits.