The standard molar entropy of NH3 is 192.45 J K1 mol at 298K, and its heat capacity is given by the equation Coma +bT +c/T2 with the coefficients given in the table below. Calculate the standard molar entropy of NH3 at 100 °C p,m Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc. Table 1: Temperature variation of molar heat capacities, Cp,m/U K-1mol-1) a + bT + c/T2 b/(10-3 K-) 25.1 c/(10 K2) a NH3 29.75 -155

The standard molar entropy of NH3 is 192.45 J K1 mol at 298K, and its heat capacity is given by the equation Coma +bT +c/T2 with the coefficients given in the table below. Calculate the standard molar entropy of NH3 at 100 °C p,m Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc. Table 1: Temperature variation of molar heat capacities, Cp,m/U K-1mol-1) a + bT + c/T2 b/(10-3 K-) 25.1 c/(10 K2) a NH3 29.75 -155

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 88QRT: Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with...

See similar textbooks

Similar questions

A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
Why isnt the entropy of elements in their standard pressure at normal that is, room temperatures equal to zero?
Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?
What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
The standard molar entropy of NH3 is 192.45 J K-1 mol-1 at 298K, and its heat capacity is given by the equation Cp,m = a +bT +c/T2 with the coefficients given in the table below. Calculate the standard molar entropy of NH3 at 100 ℃. Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc.
Calculate the measurable change in entropy (for the system) when the state of 2.00 mol ofdiatomic perfect gas molecules, for which Cp,m=7/2 R, is changed from 25 degrees Celsius and1.50 atm to 135 degrees Celsius and 7.00 atm. How do you rationalize the sign of the entropychange?
The molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1, andthe molar entropy of fusion under the same conditions is ΔfusSm (H2O)=22.0 J K-1 mol-1. Show that(a) ΔfusGm (H2O)=0 at 273.15 K and one atm, (b) ΔfusG,m (H2O) < 0 when the temperature is greaterthan 273.15 K, and (c) ΔfusGm (H2O) > 0 when the temperature is less than 273.15 K.
A sample of carbon dioxide that initially occupies 15.0 dm3 at 250 K and 1.00 atm is compressed isothermally. Into what volume must the gas be compressed to reduce its entropy by 10.0 J K-1?
The temperature dependence of the heat capacity of non-metallic solids is found to follow the Debye T3 -law at very low temperatures, with Cp,m = aT3. (a) Derive an expression for the change in molar entropy on heating for such a solid. (b) For solid nitrogen, a= 6.15 x 10-3 J K-4 mol-1. What is the molar entropy of solid nitrogen at 5 K?
The enthalpy of vaporization (deltaHvap) of water was experimentally determined to be 151.3 kJ for 3.72 mols of water at 100 degrees Celsius? Calculate the molar entropy of vaporaization (deltaSvap,m) of water.
Calculate the change in entropy (in J/⁰F) when 340g of ethanol (46 g/mol) is cooled from 50 to 40 ⁰C at constant pressure. Specific heat capacity of methanol at constant pressure is 112 J/mol-K.