Answered: The vapor pressure of ethanol is 58.7…

The vapor pressure of ethanol is 58.7 torr at 25 °C. Determine the vapor-pressure lowering, ΔP, of an ethanol solution that contains 0.125 mol sucrose dissolved into 1.545 mol ethanol.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 80QRT

See similar textbooks

Related questions

Q: Why does the dissolution of MgCl2 have a negative entropy value?

A: The entropy represents the randomness present in a system. The solid phase has less entropy than the…

Q: Molybdenum is BCC and has an atomic radius of 0.14nm. Calculate a value for its lattice constant a…

Q: The molar enthalpy of solid sodium hydroxide with a solution of hydrochloric acid. NaOH(s) + HCI(aq)…

Q: What are the variables in a van’t Hoff plot? K vs T K vs 1/T ln K vs 1/T ln…

A: To explain: The variables in a van't Hoff plot.

Q: State whether the entropy of the system increases or decreases in each of the following…

A: More is the disorderness present in the atoms of a substance more will be its entropy.

Q: Determine whether the statements below are true or false. I: Kp and Kc are related through the…

A: Given : We have to tell whether the statements are true or false.

Q: A student dissolves 13.7 g of sodium chloride (NaCl) in 300. g of water in a well-insulated open…

Q: In a coffee-cup calorimeter, 1.60 g of NH4NO3 is mixed with 75.0 g of water at an initial…

A: The amount of NH4NO3 added to 75.0 g of water is 1.60 g. The initial temperature and final…

Q: (1) Which ote tollowing has the lowest standard entropy (S) value? (A) N₂O4 (C) NO (B) NO (2) Which…

Q: State the relationship between the equilibrium constant, Kp , and the standard Gibbs free energy.

A: Interpretation - To state the relationship between the equilibrium constant, Kp , and the standard…

Q: The normal freezing point of n-octane 1C8H182 is -57 °C. Is there any temperature at which liquid…

A: INTRODUCTION: The freezing point is defined as the temperature of a liquid at which a liquid becomes…

Q: What can be said about the sign of the entropy when solid NaCl is dissolving in water? What can be…

Q: Two phases "a" and "b" of a pure substance are in equilibrium at some temperature and pressure.…

A: For any equilibrium to exist, there chemical potentials should be always equal. Hence ans will be…

Q: Is the dissolution of ammonium nitrate,is endorthermic or exothermic? Justify your answer

Q: Compound XY is an ionic compound that dissociates as it dissolves in water. The lattice energy of XY…

Q: Chloride solvable in water at 0°C is 542 g/L. What amounts of substance (in [mol]) of Magnesium…

A: Molar mass of MgCl2 = 95 g/mol Solubility of Magnesium chloride (MgCl2) = 542 g/L Molarity of MgCl2…

Q: For the chemical reaction O3(g) + OH(g) → 2 O2(g) + H(g), DrGq = 5.8 kJ/mol at 298 K, 0 J/mol at…

Q: The following gas phase system is at equilibrium: CCl4(g) + CH4(g) ⇄ 2 CH2Cl2(g) The pressure of…

A: The equilibrium is as follows: CCl4(g) + CH4(g) ⇄ 2 CH2Cl2(g)T = 533 K:P(CCl4) = 153 mmHgP(CH4) =…

Q: The enthalpy of solution for potassium perchlorate - KCIO4 is +51.04 kJ/mol. How many grams of…

Q: . Calculate the change in the temperature of the solution.

A: The heat of dissolution is absorbed by solution to raise its temperature. As the solution is…

Q: Compound XY is an ionic compound that dissociates as it dissolves in water. The lattice energy of XY…

A: Given: Lattice energy = -595.6 KJmol-1 Hydration energy of ions = -612.4…

Q: What is the change in enthalpy in joules when 10.5g of AgCl (143.3g/mol) dissolves in water…

Q: A student using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when…

A: Given: Temperature of the solution with calorimeter decreased = 1.10 K Mass of KNO3 added = 1.00 g.…

Q: 10.0 mol PCl3(g), 20.0 mol Cl2(g), and 40.0 mol PCl5(g) are introduced in a previously evacuated…

A: Given: moles of PCl3(g) = 10.0 moles moles of Cl2(g) = 20.0 moles moles of PCl5(g) = 40.0 moles…

Q: Does the zeta potential of colloidal particles depends on pOH

A: Zeta potential is a potential difference between dispersion medium and layer of fluid (stationary…

Q: Hexane and heptane are miscible with eachother in all proportions. In making a solution of them,…

A: Two solutions of pure compound which possess similar kind of properties are generally miscible with…

Q: A student dissolves 11.0 g of potassium hydroxide (KOH) in 200. g of water in a well-insulated open…

A: The heat capacity is the ratio of the energy supplied in the form of heat to the rise in the…

Q: Which has the greatest vapour pressure at 25°C? SiO2 CO2 H2O

A: At constant temperature, vapor pressure depends on the intermolecular forces. Vapor pressure will be…

Q: At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4 B(g)=2C(g) + 3 D(g) were…

A: Equilibrium constant in terms of pressure is defined as the product of partial pressures of products…

Q: 1. Calculate the molar heat of solution, AsolnH, for ycur salt. .

A: Given data: Mass of salt = 2.2 g Initial temperature T1 = 19.5o C Final temperature T2 = 29.5o C…

Q: The standard Gibbs free energy change at 100oC is 18.8 kJ/mol for the solubility equilibrium:…

A: Given ReactionLi3PO4 (s) → 3 Li+ (aq) + PO43-(aq)∆Grxn0 = 18.8 kJ/mole = 18800 J/moleT = 100°C =…

Q: At 25 ∘C , the equilibrium partial pressures for the reaction 3A(g)+4B(g)↽−−⇀2C(g)+2D(g) were…

Q: The reaction C6H12O6 + 6O2 → 6CO2 + 6H2O ΔHo = −1072 kJ/mol and ΔSo =…

A: For the given reaction, ∆H° = -1072 kJ /mol = -1072 × 103 J mol-1 ∆S° = 578 J K-1 mol-1 T = 37 ℃ =…

Q: the standard Gibbs Free Energy

Q: Does the entropy of the system increase, decrease, or stay the same when a solid sublimes?

A: Entropy is the measure of randomness. When the randomness increase entropy increases.

Q: Hydrogen gas burns in an atmosphere of bromine gas to produce hydrogen bromide gas according to the…

Q: What is the solubility of potassium chloride at 20 degrees Celsius?

A: The solubility of different salts in water at a particular temperature can be judged from the…

Q: The following gas phase system is at equilibrium: CCl4(g) + CH4(g) ⇄ 2 CH2Cl2(g) The pressure of…

A: Here the pressure of each of the gases given which are present at equilibrium. From the given values…

Q: Predict whether the entropy change of the system in each of the following is positive or negative.…

A: Given that - N2 (g, 10 atm) -----> N2 (g, 1 atm) Entropy is the randomness or disorder of…

Q: Determine the molality of a solution prepared by dissolving 28.60 g of glucose (C 6 H 12 O 6 ) into…

A: Mass of glucose = 28.60 g Mass of water = 250 g = 0.250 kg We need to find molality of solution.…

Q: The Gibbs energy of 12 g of ice at 0°C and 1 atm is less than (more negative) the Gibbs energy of…

Q: t 34.0 °C, the vapor pressure of octane is 9.5 kPa, and at 95.8 °C, its vapor pressure is 98.0 kPa.…

A: When the vapor pressure and enthalpy of vaporization studied together, they come under “Clausius…

Q: What is the molality of the solution when 0.75 mol NaCl is dissolved in 1.23 kg water? a. 0.095 m…

A: Molality - It is defined as the number of moles of solute per kilogram of solvent. Its SI unit is…

Q: (a) Adsorption of a gas on surface of solid is generally accompanied by a decrease in entropy, still…

A: A reaction is said to be spontaneous ∆G for the reaction is negative.

Q: As expected, there is an increase in entropy for this dissolution process and AS rxn is 43.4 J/K.…

A: Given, Temperature = 25°C=(25+273)K=298 K

Q: How is the solubility of oxygen in water affected by increasing temperature?

A: The gases are soluble in liquid and the solubility of a gas in a liquid depends on the nature of gas…

Q: Calculate the vapor pressure of ethnaol at 25 Celsius. Assume the thermodynamic values are…

Q: The normal freezing point of n-octane 1C8H182 is -57 °C. In what temperature range is it a…

A: The importance of Gibbs energy is that it gives information about the spontaneity of the reaction or…

Q: The following gas phase system is at equilibrium: CCL4(g) + CH4(g) 22 CH,Cl½(g) The pressure of each…

A: The relationship between ΔG i.e Gibbs free energy change and equilibrium constant (K) is given by…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

The vapor pressure of ethanol is 58.7 torr at 25 °C. Determine the vapor-pressure lowering, ΔP, of an ethanol solution that contains 0.125 mol sucrose dissolved into 1.545 mol ethanol.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
Maple syrup sap is 3% sugar (sucrose) and 97% water bymass. Maple syrup is produced by heating the sap toevaporate a certain amount of the water. (a) Describe what happens to the composition and boilingpoint of the solution as evaporation takes place. (b) A rule of thumb among maple syrup producers is thatthe finished syrup should boil about 4 C higher than theoriginal sap being boiled. Explain the chemistry behindthis guideline. (c) If the finished product boils 4 C higher than the originalsap, calculate the concentration of sugar in the finalproduct. Assume that sugar is the only solute and theoperation is done at 1 atm pressure.
14. Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies. Which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute- solvent interactions are the same for both solids. (A) The solid with the larger lattice energy, if entropy increases as a result of mixing, and the solid with the smaller lattice energy, if entropy decreases as a result of mixing. (B) The solid with the smaller lattice energy, if entropy increases as a result of mixing, and the solid with the larger lattice energy, if entropy decreases as a result of mixing. (C) The solid with the smaller lattice energy. (D) The solid with the larger lattice energy. (E) They will have the same or very similar solubilities.
Consider the following reaction at 25°C: 3 Ni(s) + N²(g) + 3 H2O(g) → 3 NiO(s) + 2NH:(g) where K = 6.74 x 104 At what partial pressure of ammonia will one be able to get out 11.5 kJ/mol of Gibbs free energy from this reaction when the rest of the mixture contains 57.6 g NiO, 182.3 g Ni, 8.54 atm of nitrogen gas, and 10.07 atm of water vapor? (Enter the partial pressure using two significant figures.)
The salt barium bromide is soluble in water. When 9.82 g BaBr2 is dissolved in 115.00 g water, the temperature of the solution increases from 25.00 °C to 26.68 °C. Based on this observation, calculate the dissolution enthalpy, ΔdissH, of BaBr2.Assume that the specific heat capacity of the solution is 4.184 J g-1 °C-1 and that the energy transfer to the calorimeter is negligible.
Provide the formal definition of enthalpy and explain all symbols used in it. Explain how the change in enthalpy is related to certain thermodynamic property (other than Gibbs energy).
sketch how the entropy of water changes as it is heated from -50 °C to 110 °C at sea level. Show the temperatures at which there are vertical increases in entropy
With the help of a suitable enthalpy cycle explain what happens when an ionic compound such as NaCl dissolves in water.
10.0 g ZnCl2 is dissolved in 100.0 g of water at 23.6 °C. The solution reaches a temperature of 36.5 °C. What is the molar heat of dissolution for ZnCl2? Assume the specific heat capacity of the solution is the same as pure water, 4.184 J/g·°C.
an aqueous iron(III) chloride solution containing 2.01 x 102 g of water that has a boiling point of 102 ° C (Assume that Kp = 0.512 °C m for water.)
3) Camphor (CoH160) melts at 179.8 °C, and it has a particularly large freezing point depression constant of 40.0 "C/m. When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.10 g of liquid camphor, the freezing point of the mixture is found to be 176.7 C. What is the molar mass of the organic substance?
Calculate the enthalpy of solution for the dissolution of lithium iodide, LiI, molar mass = 133.85 g mol-1. When 1.49 g of LiI is dissolved in a coffee cup calorimeter containing 75.0 mL of water the temperature increased from 23.5 °C to 25.7 °C. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1. -62 kJ mol-1 -39 kJ mol-1 30 kJ mol-1 -76 kJ mol-1 18 kJ mol-1