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

300 ml of 0.05 M ammonia solution, where the density of the solution is 0.88 g/ml. What is the number of moles of ammonia? What is the weight (in grams) of ammonia? What is the molality of the solution?
A solution is prepared by dissolving 11.622 g sulfuric acid, H2SO4, (Molar Mass = 98.07848 ) in enough water to make 100.0 mL of solution. If the density of the solution is 1.115 g/mL, what is the molality? Report your answer using three decimal places.
2. The concentrated sulfuric acid that we use in the laboratory is 98.0% H¿SO, by mass. Calculate the molality and molarity of the solution. The density of the solution is 1.83g/mL.
A 2.350×10−2 M solution of glycerol ( C3H8O3 ) in water is at 20.0 ∘C . The sample was created by dissolving a sample of C3H8O3 in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.0 mL . The density of water at 20.0 ∘C is 0.9982 g/mL . Part A: Calculate the molality of the glycerol solution. Part B: Calculate the mole fraction of glycerol in this solution. Part C:Calculate the concentration of the glycerol solution in percent by mass. Part D: Calculate the concentration of the glycerol solution in parts per million by mass. Please type answer note write by hend.
When 4.30 g4.30 g of a nonelectrolyte solute is dissolved in water to make 935 mL935 mL of solution at 24 °C,24 °C, the solution exerts an osmotic pressure of 885 torr.885 torr. 1.What is the molar concentration of the solution? 2.How many moles of solute are in the solution? 3.What is the molar mass of the solute?
A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 0.750 atm at 25.0°C. What is the molecular weight of the unknown solute (R = 0.0821 L•atm/K•mol)?
An aqueous CaCl2 solution has a vapor pressure of 81.6 mmHg at 50 degrees celsius. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent?
A solution of H2SO4(aq) with a molal concentration of 1.66 ? has a density of 1.104 g/mL. What is the molar concentration of this solution?
An aqueous solution of C6H₁2O6 contains 0.721 M СC6H₁2O6 (aq). The density of the solution is 1.065 g/mL. The molality of C6H12O6 in this solution is Please report molality to 3 significant figures. m. An aqueous solution of C6H₁2O6 contains 0.427 m C6H₁2O6 (aq). The mass percent of C6H₁2O6 in this solution is %. Please report mass percent to 3 significant figures.
A 6.42% (w/w) Fe(NO3)3 (241.81 g/mol) solution has a density of 1.059 g/mL. Calculate the molar concentration of this solution. In winter, after a snowstorm, salt (NaCl) is spread to melt the ice on roads. How many grams of salt per 1000. g of ice is needed to make it liquid at negative 5 space degree C ?
A solution is prepared by dissolving 4.78 g of an unknown nonelectrolyte in enough water to make 375 mL of solution. The osmotic pressure of the solution is 1.33 atm at 27°C. What is the molar mass of the solute? (R = 0.0821 L×atm/mol×K)
How many grams of CaCl2 are there in 197 grams of an aqueous solution that is 10.2 % by weight CaCl2. |g CaCl2