Answered: 14. For mercury, the enthalpy of…

14. For mercury, the enthalpy of vaporization is 58.51 kJ/mol and the entropy of vaporization is 92.92 J/°C'mol. What is the normal boiling point of mercury?

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 42E: For mercury, the enthalpy of vaporization is 58.51 kJ/mol and the entropy of vaporization is 92.92...

See similar textbooks

Related questions

Q: 12. For mercury, the enthalpy of vaporization is 58.51 kJ/mol and the entropy of vaporization is…

Q: silicon, Si, the heat of vaporization at its normal boiling point of 2355 °C is 297.1 kJ/mol. The…

A: The question is based on the concept of chemical thermodynamics. we have to calculate entropy of…

Q: What is the entropy change for the universe, delta Suniv, for the vaporization of one mole of CH3OH…

A: The solution is as follows :

Q: chapter 12: 16) The following reaction has these standard thermodynamic parameters: ΔHºrxn =…

A: Given; ΔHºrxn = –32.6 kJ/mol. ΔSºrxn = –63.8 J(mol • K). C(g)+D(g)--->E(g).

Q: When solid sodium chloride is cooled from 25°C to 0.°C, the entropy change is –4.4 J/mol. K. Is this…

A: Entropy is a measure of the degree of disorder or randomness in a system. It is a thermodynamic…

Q: Consider the following reaction: 2 NO(g) N2(g) + O2(g) The enthalpy change at 298 K for this…

A: The given equilibrium reaction is 2 NO(g) ----------> N2(g) + O2(g) The enthalpy change at 298…

Q: The enthalpy for a certain process is 121.9 kJ/mol and the entropy for the process is 454.8 J/K. At…

A: We are given that, ∆H = 121.9 KJ/mol = 121.9 × 10^3 J/mol ∆S = 454.8 J/K

Q: he boiling point of a certain pure liquid is 71.5°C and the enthalpy of vaporization is 26.5 kJ/mol…

A: According to Gibbs formula ∆G = ∆H - T∆S at equilibrium i.e Vaporization liquid ⇔ Vapour ∆G…

Q: certain substance has an enthalpy of fusion of 4.73 kJ/mol and an entropy of fusion of 21.2 J/mol/K.…

A: We know ∆H=∆S×T ∆H=4730j/mol ∆S=21.2j/mol/k So T=4730÷21.2=223.11k

Q: The boiling point of a substance is 35.0 degrees C and its heat of vaporization is 27.5 kJ/mol.…

A: Given-> Boiling point = 35°C = 35 + 273 = 308 K Heat of vaporization (∆Hv) = 27.5 KJ/mole ∆Hv =…

Q: A process increases the entropy of the system by 128 J/mol K and absorbs 54 kJ/mol of heat from the…

A: Given: Change in entropy (∆S) = 128 J/mol•K Absorbed heat=54 kJ/mol =54×103 J/mol To determine…

Q: Determine the entropy change, in J/mol K, for the vaporization of 75.0 g of liquid O2 into gaseous…

A: Temperature at which liquid O2 converts into gaseous O2 is = - 183°C∆Hvaporization for O2 = 6.820…

Q: For cesium, the enthalpy of vaporization is 68.31 kJ/mol and the entropy of vaporization is 102.3…

A: we need to calculate normal boiling point of cesium

Q: For magnesium, Mg, the heat of fusion at its normal melting point of 649 °C is 9.0 kJ/mol. The…

A: Ans Heat of fusion is the amount of heat added when one mole of solid convert to the liquid. Heat of…

Q: Hexafluorobenzene (C6F6) has an enthalpy of vaporization of 31.7 kJ/mol at its boiling point…

A: Given Enthalpy of vaporization ( ∆Hvap) = 31.7 KJ/mole 1 KJ = 1000 Joule 31.7 KJ = 31.7 ×…

Q: For rubidium, the enthalpy of vaporization is 75.82 kJ/mol and the entropy of vaporization is 110.1…

A: Enthalpy of vaporization (∆H) = 75.82 kJ/mol = 75820 J/molEntropy of vaporization (∆S) = 110.1…

Q: A metal alloy melts with an enthalpy change of 75 kJ/mol and an entropy change of 133.0 J/K.mol.…

A: For the melting of alloy, Enthalpy change (∆H) = 75 kJ/mol…

Q: In freezing a mole of liquid water at the freezing point; the enthalpy of fusion is 6.0lkJ/mol…

A: The enthalpy of fusion is 6.01 KJ/mol To determine : entropy of system , surrounding and universe

Q: The enthalpy change for a certain reaction is -209.4 kJ and the entropy change is 585.7 J/K. What…

Q: The heat of vaporization of methanol, CH3OH, is 35.20 kJ/mol. Its boiling point is 64.6°C. What is…

A: The change in entropy for the vaporization of methanol has to be calculated, Given: The heat of…

Q: For magnesium, Mg., the heat of fusion at its normal melting point of 649 °C is 9.0 kJ/mol. The…

A: When a solid melts to the liquid state its entropy increases. The entropy of fusion of the solid is…

Q: Steam is condensed at 100 , and the water is cooled to 0 and frozen to ice. What is the molar…

A: Entropy change is given by ∆S=∆H/T ,where ∆H is change in enthalpy and T is temperature.

Q: 9. The standard enthalpy of vaporization of methanol is 35.2 kJ/mol at its normal boiling point,…

A: When a liquid changes to a vapor state the entropy of the system increases. The entropy of…

Q: The entropy of vaporization for a certain organic compound is 28.1 J/Kmol, and the boiling point is…

A: given data entropy of vaporization 28.1 J/kmol boiling T=51.7 ;c find out enthalpy of vaporization

Q: What is the change of entropy in the vaporization of 5 grams of ice cube at 0C to steam at 100 C.…

A: The degree of randomness of the system is called entropy. Specific heat capacity of water(c)=…

Q: 5. The entropy change of the process H2O (s) H2O () is 22 J/K at 0 °C. Calculate the enthalpy of…

A: H2O(s)↔H2O(l)∆H=22J/KT=0∘C=0+273K=273K∆S=∆HT

Q: For a reaction ΔH= -4.7 kJ and ΔS= -69.5 J/K at 25 oC. Determine the ΔG for this reaction

A: The question is solved using Gibbs – Helmoholtz equation.

Q: From the values of ΔH and ΔS, predict which of the following reactions would be spontaneous at 25°C:…

A: The spontaneous nature of the reaction is determined by calculating the change of free energy of the…

Q: For lead, Pb, the heat of vaporization at its normal boiling point of 1740 °C is 177.8 kJ/mol.The…

A: Calculate entropy of vaporization of Pb: 1 kJ = 1000 J

Q: For water, H2O, the heat of vaporization at its normal boiling point of 100 °C is 40.7 kJ/mol. The…

A: The heat of vaporization of the water at its boiling point is = 40.7 kJ/mol The moles of water is…

Q: The standard enthalpy change and standard entropy change for the reaction are: AHP = -1036.0 kJ mol1…

Q: The enthalpy for a certain process is 146.4 kJ/mol and the entropy for the process is 463.6 J/K. At…

Q: For a given reaction, ΔH = +31.15 kJ/mol and ΔS = +126.83 J/K · mol. Above what temperature is the…

Q: The boiling point of a certain pure liquid is 78.9°C and the enthalpy of vaporization is 46.4 kJ/mol…

Q: What is the entropy change when 1.90 moles of CHCl3 condenses at 61.0 °C? [AH(vap) = 29.6 kJ/ mol at…

A: As per the given question, change in entropy needs to be calculated for condensation of chloroform…

Q: 13) Chlorofluorocarbons (CFCs) are no longer used as refrigerants because they help destroy the…

A: We have boiling point of CCl3F as 23.8°C, also molar heat of vaporization is 24.8 kilo joule per…

Q: . Chloroform, CHC13, has a normal boiling point of 61 °C and it enthalpy of vaporization is 29.24…

A: Formula used:- ∆G°=∆H°-T∆S° But in this condition ∆G° = 0 Thus new formula is ∆S° = ∆H°/T

Q: Consider the reaction below for the decomposition of carbon tetrachloride gas: CCl4(g) ------>…

Question

14. For mercury, the enthalpy of vaporization is 58.51 kJ/mol and the entropy of vaporization is 92.92 J/°C'mol. What is the
normal boiling point of mercury?

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

How does the second law of thermodynamics explain a spontaneous change in a system that becomes more ordered when that process is exothermic?
Which contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.
One statement of the second law of thermodynamics is that heat cannot be turned completely into work. Another is that the entropy of the universe always increases. How are these two statements related?
What happens to the entropy of the universe during a spontaneous process?
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
When solid sodium acetate crystallizes from a supersaturated solution, can you accurately predict the sign of H for the crystallization? Why or why not?
The combustion of acetylene, C2H2, is a spontaneous reaction given by the equation 2C2H2(g)+5O2(g)4CO2(g)+2H2O(l) As expected for a combustion, the reaction is exothermic. What is the sign of H? What do you expect for the sign of S? Explain the spontaneity of the reaction in terms of the enthalpy and entropy changes.
10.104 (a) When a chemical bond forms, what happens to the entropy of the system? (b) Thermodynamically, what allows any bond formation to occur? (c) What do your answers to parts (a) and (b) suggest must be true about the formation of chemical bonds for the octet rule to hold?
Some water is placed in a coffee-cup calorimeter. When 1.0 g of an ionic solid is added, the temperature of the solution increases from 21.5C to 24.2C as the solid dissolves. For the dissolving process, what are the signs for Ssys, Ssurr, and Suniv?
Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universe
Thermodynamics provides a way to interpret everyday occurrences. If you live in northern climates, one common experience is that during early winter, snow falls but then melts when it hits the ground. Both the formation and the melting happen spontaneously. How can thermodynamics explain both of these seemingly opposed events?
Consider the reaction of 2 mol H2(g) at 25C and 1 atm with 1 mol O2(g) at the same temperature and pressure to produce liquid water at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?