B.The molal boiling point elevation constant K, =0.80 °C-kg mol for a certain substance X. When 87.1 g of urea((NH), CO) are dissolved in 750. g of X,the solution boils at 149.0 °C. Calculate the boiling point of pure X.Round your answer to 4 significant digits.5.ContinueSubmit AssignmentO 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center AccessibilityMacBook ProA#&$4*3.7.altoptioncommandoption

Given : kb for X = 0.80°C.kg-1.mol-1 Mass of urea = 87.1 g Mass of X = 750.0 g Boiling point of…

(NEL), CO) 1 The molal boiling point elevation constant K =0.80 °C-kg mol for a certain substance X. When 87.1 g of urea are dissolved in 750. g of X, the solution boils at 149.0 °C. Calculate the boiling point of pure X.

(NEL), CO) 1 The molal boiling point elevation constant K =0.80 °C-kg mol for a certain substance X. When 87.1 g of urea are dissolved in 750. g of X, the solution boils at 149.0 °C. Calculate the boiling point of pure X.

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

Related questions

Q: What is the mole fraction of benzene, C6H6, in the vapor phase from a solution consisting of a…

A: vapour pressure of benzene = 768 torr vapour pressure of toluene = 283 torr Mole fraction of…

Q: The molal freezing point depression constant K = 3.50 °C-kg-mol X, the solution freezes at -8.0 °C.…

A: Consider the given information as follows;

Q: 4. A 16.0 °C. Determine the solubility in g solute/100 g H₂O. Determine the mole fraction of solute…

A: Answer: Saturated solution is the type of solution in which no more solute can be dissolved in…

Q: Now a solution is prepared by dissolving solid FeCl3 ( molar mass = 162.2 g/mol)in water. If the…

A: Given that: Mass percentage = 26.0 % Density of solution = 1.25 g/mL…

Q: The normal freezing point of a certain liquid X is 1.60 °C, but when 18.2 g of benzamide (C₂H,NO)…

Q: K,= 2.57 °C kg mol for a certain subs 20 colution freezes at 5.7 °C. Calculate the freezing point of…

A: At freezing point of liquid there exists equilibrium between solid particles and solvent phase.…

Q: The normal freezing point of a certain liquid X is -2.7 °C, but when 12.2 g of urea ((NH,),CO) are…

Q: The normal freezing point of a certain liquid X is -4.4 °C, but when 12.06 g of urea freezes at -8.3…

A: The normal freezing point of a certain liquid X is -4.4o CWhen 12.06 g of urea is dissolved in 350…

Q: The normal freezing point of a certain liquid X is -0.70 °C, but when 19. g of sodium chloride…

A: Given ,Normal freezing point of certain liquid, X Mass of NaCI = 19. gMass of X = 850. gObjective…

Q: The normal boiling point of a certain liquid X is 133.8 °C, but when 65. g of urea ((NH,),CO) are…

Q: The vapor pressure of chloroform is 173.11 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that…

A: Given Vapor pressure Chloroform = 173.11 mmHg Mass of aspirin ) = 10.87 gram Molar mass of…

Q: What mass of ethylene glycol, when mixed with 225 g H2O, will reduce the equilibrium vapor pressure…

A: To solve this problem we have to calculate the mass of the solute (ethylene glycol). Raoult's Law of…

Q: What is the total equilibrium vapor pressure of a benzene toluene solution if the mole fraction of…

Q: What would be the theoretical freezing point of a solution made by dissolving 5.551 g of CrSO 4 in…

A: Depression of freezing point is a colligative property which depends upon the concentration of…

Q: The vapor pressure of an aqueous solution of silver nitrate at 27 °C is 0.03456 atm. The vapor…

A: Answer:Properties of a solution that depend upon the number of solute particles present in solution…

Q: A certain substance X melts at a temperature of 7.4 °C. But if a 350. g sample of X is prepared with…

A: To calculate the molal freezing point depression constant Kƒ of substance X, we first need to…

Q: 5.152g of Na2CO3(s) is added to 75.0mL of water at 21.20°C. When the dissolution is complete, the…

A: Molarity of the solution can be calculated by using Following formula - Molarity = mass×1000/molar…

Q: A solution contains 3.95 g of carbon disulfide (CS2) and 2.43 g of acetone (CH3COCH3). At 35 °C the…

A: The mole fraction of carbon disulphide is calculated as shown below.

Q: A chemistry student weighs out 0.036 kg of an unknown solid compound X and adds it to 150. mL of…

A: Given that 0.036 kg of an unknown solid compound X is added to 150 mL of water at 17°C.After 10…

Q: - 1 The molal freezing point depression constant K₁=2.02 °C-kg-mol for a certain substance X. When…

Q: .9720 M aqueous solution of NaCl has a density of 1.03625g/cm^3 at 25 C, Calculate the molality of…

A: As per our guideline we can solve only one question at a time, please post other questions as next…

Q: The molal freezing point depression constant K,=4.05 °C - kg • mol for a certain substance X. When…

Q: When 1.504 g of solte is dissolved in 5.012 g of solvent (benzene), the solution freezes at -7.05 C.…

Q: The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves…

A: Since you have posted multiple questions, we will provide the solution only to the first five…

Q: A certain liquid X has a normal freezing point of -4.00 °C and a freezing point depression constant…

Q: at a particular temperature the solubility of co2 in water is 0.13 m when the partial pressure is…

A: Henry law: This law states that the concentration of a gas dissolved in a liquid depends on the…

Q: A solution is made by adding 0.978 mol sucrose to 250.0 g water. Calculate the boiling point of this…

A: Change in the intermolecular forces of a solvent by mixing of impurities as solutes results in an…

Q: When 498. mg of a certain molecular compound X are dissolved in 25.0 g of dibenzyl ether…

A: A numerical problem based on properties of liquids. A set of data for depression of freezing point…

Q: When 571. mg of a certain molecular compound X are dissolved in 60.0 g of benzene (CH), the freezing…

Q: The solubility limit of a solute at 20. °C and 1.0 atm is 13.8 g of solute per 1 L of water. What…

A: The explanation is given below-

Q: A student prepares a solution by dissolving 2.09 g of para-dichlorobenzene (C6H4Cl2,= 147.0 g/mol)…

Q: Important válues if needed for this question. The freezing point of benzene, CH, is 5.500 °C at 1…

A: Given : Boiling point of pure benzene i.e solvent = 5.500 oC Kf of benzene = 5.12 oC/m Boiling point…

Q: A certain liquid X has a normal freezing point of −6.30°C and a freezing point depression constant…

Q: What is the freezing point (in K) of a solution made by dissolving 11.983g of CCl4 in 130.0 g of…

A: Given, Mass of CCl4 solute = 11.983 g Mass of benzene solvent = 130.0 g = 0.130 kg Freezing point of…

Q: A certain substance X has a normal freezing point of 1.5 °C and a molal freezing point depression…

Q: 1. A 0.735 g of a covalent organic compound is dissolved in 15.00 g cyclohexane (freezing point =…

A: The depression in freezing point is given by, ΔTf = mKf…

Q: The normal freezing point of a certain liquid X is 0.10 °C, but when 18. g of potassium bromide…

Q: The vapor pressure of an aqueous solution of copper(II) sulfate at 38 °C is 0.06430 atm. The vapor…

Q: 16. Calculate the vapor pressure of a solution prepared by dissolving 0.750 mol of a non-volatile…

A: No. of moles of hexane,n = = = 3.77 molNo . of moles of non-volatile solute , n' = 0.750 molTotal no…

Q: The vapor pressure of an aqueous solution of iron(III) chloride at 32 °C is 0.04587 atm. The vapor…

A: Depression in freezing point, elevation in boiling point, lowering of vapor pressure etc. are…

Q: What would be the theoretical freezing point of a solution made by dissolving 15.56 g of CrSO 4 in…

Q: 3. If a solution is made up by mixing 6.0 g of benzoic acid in 1.00 L of water at 42 °C, would the…

A: In this question we have to define the saturated Solution of the benzoic acid and water, first of…

Q: a) Calculate the freezing point of a solution containing 13.2 gg FeCl3FeCl3 in 156 gg water. b)…

A: Three numerical problems based on colligative properties, which are to be accomplished.

Q: A solution is prepared by adding 425g of AgNO3 to 0.150L of water at 40.0∘C. The solubility of AgNO3…

A: The solubility of a compound is the dissolution of a solute in the solvent. It is measured in the…

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

B.
The molal boiling point elevation constant K, =0.80 °C-kg mol for a certain substance X. When 87.1 g of urea
((NH), CO) are dissolved in 750. g of X,
the solution boils at 149.0 °C. Calculate the boiling point of pure X.
Round your answer to 4 significant digits.
5.
Continue
Submit Assignment
O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility
MacBook Pro
A
#
&
$4
*
3.
7.
alt
option
command
option

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 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

A certain liquid X has a normal freezing point of -6.90 °C and a freezing point depression constant K=3.91 °C·kgmol . Calculate the freezing point of a solution made of 146.g of iron(III) chloride (FECI,) dissolved in 900. g of X. Round your answer to 3 significant digits.
A certain liquid X has a normal freezing point of -3.00 °C and a freezing point depression constant 2.24 °C.kg mol . A solution is prepared by dissolving some ammonium chloride (NH,Cl) in 450. g of X. This K=2 solution freezes at -4.2 °C. Calculate the mass of NH Cl that was dissolved, Be sure your answer is rounded to the correct number of significiant digits. Oxto S.
What is the mole fraction of acetone, C3H6O, in the vapor phase from a solution consisting of a mixture of acetone and ethyl acetate, CH3COOCH2CH3, at 30.00 °C, if the total pressure above the solution is 202.2 torr? The vapor pressures of pure acetone and NaN at 30.00 °C are 285.0 torr and 118.0 torr, respectively.
The normal freezing point of a certain liquid X is 4.60°C, but when 40.g of iron(III) nitrate (FeNO33) are dissolved in 350.g of X the solution freezes at 3.7°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Be sure your answer is rounded to the correct number of significiant digits.
Determine the boiling point (in °C) of a solution that contains 45.5 g of MgCl2 dissolved in 685 mL of ethanol (density = 0.789 g/mL). Pure ethanol has a boiling point of 78.3°C and a Kp = 1.07°C/m. %3D
1 for a certain substance X. When 38.6 g of urea (NH,), CO) The molal boiling point elevation constant K, =1.54 °C·kg mol are dissolved in 950. g of X, the 9. 2 solution boils at 113.3 °C. Calculate the boiling point of pure X. Round your answer to 4 significant digits. x10
The normal freezing point of a certain liquid X is 0.60°C, but when 0.14 kg of barium hydroxide (BaOH2) are dissolved in 900.g of X the solution freezes at −1.6°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Round your answer to 2 significant digits.
Use the solubility curve below to determine how much NaNO, can dissolve in 300 g of water at 10 degrees Celsius. 100 90 NANO, 80 70 60 CaCl 50 Pb(NO)2 40 KCI NaCi 30 20 KCIO, 10 Ce,(SO 10 20 30 40 50 60 70 80 90 100 Temperature (°C) O 240 g O 160 g O 40 g O 80 g Solubility (g of salt in 100 g H,O) EONY K,Cr,O,
The vapor pressure of an aqueous solution of barium chloride at 26 °C is 0.03172 atm. The vapor pressure of pure water at the same temperature is 0.03316 atm. Estimate the freezing point of the solution. For water, Kfp = 1.86 °C/m. °C
The molal boiling point elevation constant K = 1.15 °C·kg⋅mol the solution boils at 145.4 °C. Calculate the boiling point of pure X. Be sure your answer has the correct number of significant digits. °C x10 1 for a certain substance X. When 14.4 g of urea Ś ((NH,),CO) (NH₂) CO) are dissolved in 150. g of X,
A certain organic compound O has a solubility in acetonitrile of 13.8 at 25. °C. Calculate the mass of O that's dissolved in L 650. mL of a saturated solution of O in acetonitrile at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits. x10
The normal boiling point of a certain liquid X is 121.00 °C, but when 0.12 kg of benzamide (C,H,NO) are dissolved in 800. g of X the solution boils at 122.9 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Be sure your answer is rounded to the correct number of significiant digits. °C· kg x10 K, = || mol