Chemical Thermodynamics Puns

[Request] Introduction to Chemical Engineering Thermodynamics 9th edition

Smith, J. M.,van Ness, H. C.,Abbott, M. M.,Swihart, M. T.,"Introduction to Chemical Engineering Thermodynamics," 9th ed., McGraw-Hill, New York, 2022.

ISBN: 978-1-260-72147-8

Previous vouches are in earlier mixed post .!

Discord tag : ➡️➡️ C-137SHIVAM#4791

I’ve noticed that many engineering courses require thermodynamics, but is it really all that necessary?

Wouldn’t a typical physics course in thermodynamics suffice since you can basically apply that knowledge to any field of study that requires it?

Adsorptive chemical separation is at the forefront of future technologies, to be used in chemical and petrochemical industries. In this process, a porous adsorbent selectively allows a single component from a mixture of three or more chemical components to be adsorbed or permeate. To separate the unsorted chemicals, a different adsorbent is needed. A unique adsorbent which can recognize and separate each of the chemicals from a mixture of three or more components is the necessity for the next generation porous materials. In this regard, we demonstrate a “dynamic chemical clip” in a supramolecular framework capable of thermodynamic and kinetics-based chemical separation. The dynamic space, featuring strong preference for aromatic guests through π-π and C-H···π interactions and adaptability, can recognize the individual chemical isomers from mixtures and separate those based on thermodynamic and kinetic factors. The liquid-phase selectivity and separation of the aromatic isomers are possible by the adaptability of the “chemical clip” and here we elucidate the prime factors in a combinatorial approach involving crystallographic evidence and detail computational studies.

https://ift.tt/3zltyOA

Does anybody know of a school that is offering Thermo 2 online for Chemical Engineers? I have been looking around online, and I either find schools that don't have Thermo 2, don't offer it online, or don't offer it over the summer. If you have any information on whether your school offers it or of a school that does please let me know.

I started doing a BSc but I got accepted into engineering on Friday night. I've ordered all the other books I need but the ENGGEN 140 book is out of stock at the moment and it is crucial for this semester. I'm happy to pay the same price as a new one as well

Need help ASAP on 1.5 hr test. $100

hello,

can you please share some websites and book titles on chemical thermodynamics, i'm getting a little bit confused because a simulation i'm running on a thermal recovery device on an ICE with a proprietary fuel is yielding excessive amounts of energy, i'm getting all sorts of results (ammonia emissions !?)

thank you in advance

Test will be on Power cycles, Refrigeration, Introduction to VLE, Ideal/Nonideal Mixtures, Vapor - liquid equilibria. Will test knowledge beforehand to negate possibility of scam. Price Negotiable. Half Before and Half After Grade comes out. KaptainYes#3719

I need to practice questions for my exam, if possible, can anyone provide me with solution manual? 8th Edition would be preferable.

Hello,

I recently found this community bc they helped me find a book I needed, so I decided to give back to y'all, if any of you need, here is the book.

I am stuck on this problem. I already did the first part, but I don't know how to do the second one. Help me pls

1.Assuming that the heat capacities of substances are independent of temperature, calculate ∆rH°=391.40 for the reaction:

CH3COOH (g) + 2O2 (g) → 2H2O (g) + 2CO2 (g)

Given the following data:

https://preview.redd.it/xeecv6pa5cy51.png?width=543&format=png&auto=webp&s=3333819c80ad521a9daef06752d0fc34ee0b7053

2. How the spontaneity of the process is affected when the reaction is carried out at 391.40 K, with respect to when it is carried out at 298.15 K? Note: Consider the phases in which substances are found at both temperatures.

Any Chemical engineers willing to help on a open book thermodynamics exam I have to take in december.

I've googled this many times and asked my professor, however, I'm still a bit confused on what standard state Gibbs Free Energy actually represents in relation to a chemical system's spontaneity and thermodynamic properties. Specifically, I'm referencing the (simplified) equation G = Enthalpy - (Temperature*Entropy), not the energy of a Galvanic cell.

I understand why the energy change of a system is the sum of heat and work, but what makes this different from Gibbs Free Energy, and why do we subtract the product of entropy and temperature from enthalpy?

For reference, I'm a chemical engineering undergrad in their first year of studies.

Smith, J. M.,van Ness, H. C.,Abbott, M. M.,Swihart, M. T.,"Introduction to Chemical Engineering Thermodynamics," 9th ed., McGraw-Hill, New York, 2022.

ISBN: 978-1-260-72147-8

I need you to take my Chemical Engineering thermodynamics I BS level.