Q: Discuss Temperature Variation of Entropy?
A: Given : To discuss temperature variation of entropy.
Q: ate the molar entropy of a
A:
Q: The variation of free energy with pressure at constant temperature is given by
A:
Q: Estimate molar entropy of kcl at 5K given that it's molar heat capacity at that temperature is…
A:
Q: With a typical example, explain the concept of residual entropy
A: The difference in entropy of a substance between its non-equilibrium state and its crystal state…
Q: Estimate the molar entropy of potassium chloride at 5 .0 K given that its molar heat capacity at…
A:
Q: When a gas undergoes reversible adiabatic expansion, its entropy remains constant even though the…
A:
Q: Calculate the entropy of a two chambered system with six particles if Boltzmann constant is 1.38 *…
A: Given that no. Of particles = N = 3 Kb = 1.38 x 10-23 J/K No. Of microstates = W
Q: 2.) Calculate the entropy for parking in a parking lot with 10 parking spots, assuming you can park…
A: Entropy is the degree of disorderness or randomness in a system. To calculate entropy, Boltzmann…
Q: How can i know what's entropy?
A: Entropy is a thermodynamic concept, as well as a measurable physical property that is most commonly…
Q: Calculate the standard state entropy of formation for H2O gas and of H2O liquid. Why is the entropy…
A: Solution: Standard entropy values at 25 deg. C for reference
Q: Two ideal gases under same pressure and temperature are allowed to mix in an isolated system – what…
A: SOLUTION: Step 1: In an isolated system, during mixing of gases, there is no exchange of energy or…
Q: Which of the following has the largest standard entropy (S °)?
A:
Q: Define Gibbs energy.
A: Thermodynamics is the study of effects of work, heat and energy on a system. It basically tells how…
Q: The molar entropy of a sample of neon at 298 K is 146.22 J K−1 mol−1. The sample is heated at…
A:
Q: molar entropy for t
A:
Q: The standard entropy of ammonia gas at 298.15 K is 192.77 J/K/mol. Calculate the entropy of 6.487…
A: Given, Standard entropy= 192.77 J/K/mol Temperature= 298.15 K Boiling point= -33.34 C = 239.8 K To…
Q: 1.1 State the first law of thermodynamics 1.2. What is the difference between isobaric process and…
A: 1.1 The statement for first law of thermodynamics: The total energy of an isolated system is does…
Q: Why classical theory of lattice heat capacity gives same results at High and Low temperatures
A: Classical theory of heat capacity is also known as Dulong-Petit Law.
Q: Determine the change in entropy for 1.0 mole of an ideal gas originally confined to one- half of a…
A: At constant temperature, change in entropy is calculated using formula :
Q: Determine the reversible work, in joules, for the expansion of 3.00 mol of an ideal gas from 4.0000…
A: When ideal gas expands the work is done by the system on the surrounding. The work done is given by:…
Q: Calculate the entropy for parking in a parking lot with 10 parking spots, assuming you can park in…
A:
Q: Write an equation that expresses the first law of thermodynamics in terms of heat and work. Under…
A: First law of thermodynamics is expressed by:
Q: what do you mean by reversible work. describe briefly
A: In a thermodynamic process, there can be of two types of processes namely reversible and…
Q: What is the signifi-cance of entropy being a state function?
A: Entropy is a thermodynamic state function that determines randomness in a system. When we raise…
Q: Calculate the maximum work and the maximum non-expansion work that can be obtained from the…
A:
Q: Use a Table of Thermodynamic Data to calculate the standard molar entropy change for a) the…
A:
Q: At what temperature is the standard molar entropy of helium equal to that of xenon at 298 K?
A: for monoatomic ideal gases, Sm= R lnVe52Nl3 for 1 mole N=1 Sm= R lnVe52l3 Sm= R…
Q: One mol of an ideal gas at 300 K expands reversibly from 3 x 102 m³ to 5 x 102 m3, Calculate the…
A: Entropy change at contact temperature with change of volume relation given below
Q: Calculate the entropy associated with a transition between orthorhombic sulfur and monoclinic…
A: In this question, we have to Calculate the entropy associated with a transition between orthorhombic…
Q: properties of a thermodynamic system
A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…
Q: A system contains 758 particles and has 7.96* 1032 possible configurations. What is the entropy of…
A: GivenNo of particles = N = 758 No of possible configuration = C = 7.96 * 1032 Entropy of the system…
Q: What thermodynamic properties are extensive
A: Extensive thermodynamic property: A thermodynamic property that depends upon the size or the…
Q: Derive an expression showing how entropy can be related to thermodynamic probability.
A: The relation between entropy and thermodynamic probability are given as follows:
Q: Choose the correct answer out of the three options: Suppose an isolated system undergoes a change…
A: The entropy of the system is the degree of measurement of randomness or disorderness in the system.…
Q: Fill the table with their respective standard entropy of reaction and show the solutions.
A:
Q: Suppose that you find out that a system has an absolute entropy zero. What else can you conclude…
A: The absolute entropy of a system is the entropy at absolute temperature, 0 K.
Q: Find the absolute entropy of Nitrogen gas at 100 K. Assume that the heat capacity of nitrogen gas in…
A: Answer: Entropy of system is the measure of its disorderliness or randomness. In more possible…
Q: Beginning from the Clausius inequality, derive for us several (two more) units of entropy or
A: Clausius inequality
Q: A gaseous system undergoes a change in temperature and volume. What is the entropy change for a…
A: The relation between the entropy (∆S) and the number of microstates (W) is given below in which k is…
Q: Explain “residual entropy”. Estimate the residual molar entropies for mono‐ and di‐deuterated ethane…
A:
Q: Give the mathematical expression of heat capacity.
A:
Q: Calculate the change in entropy
A:
Q: Thermodynamic state functions include enthalpy, entropy, and _____________.
A: Thermodynamic state function having four states, but here only two is given remaining has to be…
Q: Calculate a change in entropy for an irreversible process of a system and contrast with the change…
A: An irreversible process is a process that cannot return both the system and the surroundings to…
Step by step
Solved in 2 steps
- Determine an expression for V/T p, n in terms of and . Does the sign on the expression make sense in terms of what you know happens to volume as temperature changes?What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?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?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 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 standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are, respectively, -238.7 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the change in the entropy of the surroundings (in J/K) upon the combustion of 13.3 g of methanol under a constant pressure of 1.000 atm and a temperature of 25.00 oC. N.B. combustion is the reaction of this substance with molecular oxygen to produce water and carbon dioxide.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.
- A closed, but not isolated system is in thermal contact with its surroundings. The system's volume is fixed at 7.3 L. Both the system and surrounds have a temperature of 25 °C. A chemical reaction occurs inside the system for which ΔrU = 11.38 KJ. (A) What is the change in entropy for the surroundings for the process, ΔSsurr? (B) What are the ranges of possible values for the change in entropy of the system, ΔSsys , for this process?At very low temperatures the molar constant-pressure heat capacity of many solids varies as aT3, where a is an empirical constant. Suppose that for a certain solid Cp,m =0.43 J K-1 mol-1 at 4.2 K. What is the change in the molar entropy o f this solid as its temperature changes from 4 .2 K t o 10 .0 K?The standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are -238.7 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol respectively. Calculate the change in surrounding entropy (in J/K) during combustion of 12.7 g of methanol under a constant pressure of 1,000 atm at 25.00 oC (N.B., combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).