The enthalpy of vaporization of mercury is 58.5 kj/mol and the normal boiling point is 630K,...
The enthalpy of vaporization of mercury is 58.5 kj/mol and the normal boiling point is 630K, You want to calculate the entropy of vaporization for mercury. Which of the following statements concerning this problem is incorrect? Why is this statement incorrect?
A) We wxpect DS to be positive for the vaporization of mercury
B) Once we know that DS is for this process we will know if it is spontaneous
C) We can calculate the entropy of mercury because we know that DG=0 at the normal boiling point
Homework Answers
dS = q / T
dS = 58.5 * 10^3 / 630 K
dS = 92.857 J / mol K
option B: Once we know that DS is for this process we will know if it is spontaneous
spontanity of a reaction depends upon gibbs free energy if dG = -ve then it is spontaneous and dG = +ve then the reaction is endothermic.
Add Answer to:
The enthalpy of vaporization of mercury is 58.5 kj/mol and the
normal boiling point is 630K,...
The enthalpy of vaporization of trichloromethane (chloroform, CHC13) is 29.4 kJ mol-'at its normal boiling point...
The enthalpy of vaporization of trichloromethane (chloroform, CHC13) is 29.4 kJ mol-'at its normal boiling point of 334.88 K, calculate (i) the entropy of vaporization of trichoromethane at this temperature and (ii) the entropy change of the surrounding.
The enthalpy of vaporization of Substance X is 18.0 kJ/mol and it’s normal boiling point is...
The enthalpy of vaporization of Substance X is 18.0 kJ/mol and it’s normal boiling point is 146. degrees C. Calculate the vapor pressure of X at 62. degrees C.
The enthalpy is vaporization of Substance X is 14.0 kJ/mol and it’s normal boiling point is...
The enthalpy is vaporization of Substance X is 14.0 kJ/mol and it’s normal boiling point is 148 degrees C. Calculate the vapor pressure of X at 22 degrees C.
196 The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. a)...
196 The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease? b) Calculate the value of ΔS when 1.50 mol of Br2(l) is vaporized at 58.8 ∘C. ΔS= (answer in J/K)
the normal boiling point of ethanol is 78.3 deg C and its molar enthalpy of vaporization is 38.56 Kj/mol. what is the ch...
the normal boiling point of ethanol is 78.3 deg C and its molar enthalpy of vaporization is 38.56 Kj/mol. what is the change in entropy in the system in J/k when 97.2 grams of ethanol at 1 atm condenses to a liquid at the normal boiling point?
The normal boiling point of ammonia is -33.3°C, and its enthalpy of vaporization is 23.35 kJ/mol....
The normal boiling point of ammonia is -33.3°C, and its enthalpy of vaporization is 23.35 kJ/mol. Calculate the temperature in °C required to double the vapor pressure of ammonia.
1. a. The enthalpy of vaporization of liquid mercury is 59.11 kJ/mol. What quantity of energy...
1. a. The enthalpy of vaporization of liquid mercury is 59.11 kJ/mol. What quantity of energy as heat is required to vaporize 0.240 mL of mercury at 357 °C, its normal boiling point? The density of mercury is 13.6 g/mL. Energy = ____ kJ b. Determine ethanol’s normal boiling point by slowly changing the temperature to the point where the vapor pressure equals 760 mmHg. What is this temperature? °C
The normal boiling point of methanol is and the molar enthalpy of vaporization if 71.8 kJ/mol....
The normal boiling point of methanol is and the molar enthalpy of vaporization if 71.8 kJ/mol. The value of S when 1.75 mol of vaporizes at 64.7 °C is 0.372 4.24 × 107 372 1.94 × 103 1.
The standard enthalpy of vaporization (H°vap) of methylacrylate (CH2CHCO2CH3) is 36.0 kJ/mol. The normal boiling point...
The standard enthalpy of vaporization (H°vap)
of methylacrylate
(CH2CHCO2CH3) is 36.0
kJ/mol.
The normal boiling point of methylacrylate is
80.5°C.
Calculate the vapour pressure of methylacrylate at
43.0°C.
The molar enthalpy of vaporization of NH3 is 23.3 kJ/mol at its normal boiling point of...
The molar enthalpy of vaporization of NH3 is 23.3 kJ/mol at its normal boiling point of -33.3 °C. How much energy is required to evaporate 2.03 kg of ammonia at -33.3 °C?
The enthalpy of vaporization of trichloromethane (chloroform, CHC13) is 29.4 kJ mol-'at its normal boiling point of 334.88 K, calculate (i) the entropy of vaporization of trichoromethane at this temperature and (ii) the entropy change of the surrounding.
Most questions answered within 3 hours.
-
Where is the error in this code sequence?
String s1 = "Hello";
String s2 = "ello";...
asked 11 months ago -
Financial data for Joel de Paris, Inc., for last year
follow:
Joel de Paris, Inc.
Balance...
asked 11 months ago -
Consider this reaction:
Al2(SO4)3 (aq)+ BaCl3
(aq) Al2Cl6 (aq)- +
3BaSO4(s) . What is the...
asked 11 months ago -
Suppose that Savneet is considering increasing her
recent random sample from 20 car rentals to 40...
asked 11 months ago -
Trucks arrive at an unloading terminal at an average rate of 120
per hour.
Trucks arrive...
asked 11 months ago -
Why are methanol and ethanol completely soluble in water while
octanol is not very little soluble....
asked 11 months ago -
A facilities manager at a university reads in a research report
that the mean amount of...
asked 11 months ago -
When the CuSO4 is rehydrated by adding water to the anhydrous
compound, is this an endothermic...
asked 11 months ago -
A ray of sunlight is passing from diamond into crown glass; the
angle of incidence is...
asked 11 months ago -
A block of mass 0.249 kg is placed on top of a light, vertical
spring of...
asked 11 months ago -
how do the kidneys compensate in the presences of acidosis
a) trigger hyperventilate
b) reserve acid...
asked 11 months ago -
Question 501 pts
The rental rate of capital to the firm increases. Which of the
following...
asked 11 months ago