CHEMISTRY COMMUNITY

Tim Nguyen 2J

The two H atoms add a net +2 charge to the product side, so you need to add two e- to balance that out.

Tim Nguyen 2J

Gibbs Free Energy is heavily dominated by the enthalpy term. Even though entropy can be negative in terms of the system, the reaction overall can still be spontaneous as stated above by its relation to the entropy of surroundings.

Tim Nguyen 2J

You only add OH when the redox reaction is in a basic solution

Tim Nguyen 2J

Higher peaks should indicate a slower rate since it takes more energy to overcome the higher activation energy. Lower peaks are easier to overcome thus indicating a lower activation energy.

Tim Nguyen 2J

The highest peak should be the slowest step which is the rate determining step

Tim Nguyen 2J

Yeah of course! As Dr. Lavelle discussed in class, the internal energy of an isolated system is constant. Since the universe is defined as an isolated system, the summation of all the work and heat transferred in the universe is constant. Therefore the change in internal energy (delta U) of the univ...

Tim Nguyen 2J

I think that old tests and homework problems are the way to go!

Tim Nguyen 2J

Yes, because I think that this is the first law of thermodynamics where energy is neither created nor destroyed :)

Tim Nguyen 2J

I think if we are given which steps are slow or fast, the pre-equilibrium approach is the most preferred. The steady state approximation is used when we are not given the slow and fast steps and need to assume that the concentration of intermediate(s) is constant (or at a steady state) to be able to...

Tim Nguyen 2J

The catalyst provides a different path for reactants to end up at the same products. Increased collisions allow it to proceed with less energy.

Tim Nguyen 2J

The pre-equilibrium method is essentially writing the rate law for the slow step and substituting any intermediate terms with equivalents derived from previous or consequent steps' equilibrium constants.

Tim Nguyen 2J

If work is negative, the system is losing energy as it uses it to expand.

If work is positive, the system is gaining energy as it gains it from the compressing force.

Tim Nguyen 2J

Gibbs Free Energy is essentially the amount of energy available for work so deltaG is also equal to max work possible.

Tim Nguyen 2J

Yes, usually for these problemes, if it isn't stated, we should probably assume standard conditions.

Tim Nguyen 2J

Calculate the entropy of a sample of a solid in which the molecules may be found in any one of three orientations with the same energy. Suppose there are 30 molecules in the sample.

Using Boltzmann's formula, the value for W would be 30^3? How would you arrive to the answer of 4.5 x 10^-22 J/K?

Tim Nguyen 2J

Dylan Mai 1D wrote:is there an entropy of fusion?

I don't think it is a tabulated value in any of the tables or appendixes in the textbook, but you can definitely calculate it similarly to calculating the entropy of vaporization.
entropy of fusion = enthalpy of fusion/melting point (Tb)

Tim Nguyen 2J

No, electrochemistry should not be on the midterm. Dr. Lavelle said in class that the midterm would only cover material from Ch. 8,9, and 11.

Tim Nguyen 2J

Spontaneous reactions are the likely paths reactions or processes will take without an input of energy (ice melting for instance).

Tim Nguyen 2J

A steeper slope would indicate a lower heat capacity since it heats up faster with less energy; conversely, a flatter slope would indicate a higher heat capacity because the same amount of heat is heating the substance in question slower.

Tim Nguyen 2J

Along with the equation, I also just stated that energy can neither be created nor destroyed, just transferred in various forms.

Tim Nguyen 2J

Water gas is an inexpensive, low-grade fuel that can be made from coal. (a) Is the production of water gas exothermic or endothermic? In the reaction given in the problem, the reactants are carbon (s) and water vapor (g) and the products are carbon monoxide (g) and hydrogen (g). Why is the reaction ...

Tim Nguyen 2J

In general with the problems we've had, a gas doing expansion work is doing work on the surroundings (negative work in terms of the whole system). When a gas compresses, work is being done on it (so positive work since energy is being put into the system to compress the gas).

Tim Nguyen 2J

I think reading the textbook might be a good start (it seems to be helping conceptually) :)

Tim Nguyen 2J

The first law is basically conservation of energy (energy is neither created nor destroyed). The more practical application of the law that we have been using is delta U = q+w

Tim Nguyen 2J

Both units of answer seem to be appropriate, but the kJ variation would only make it neater in terms of truncating the number.

Tim Nguyen 2J

As the response stated above iterates, since you know that Krypton is assumed to behave as an ideal gas, you must refer to the molar heat capacity constants for ideal gases under constant pressure and volume (in this case, 5/2R and 3/2R respectively. Using those values in q= n(molar heat capacity un...

Tim Nguyen 2J

For this problem, I found it easier to consider the units of the enthalpy of vaporization. In the table of enthalpy of vaporization values, we are given values with units of kJ/mol. In other words, each value tells us the number of kJ it takes to vaporize 1 mol of said substance. In both parts a and...

Tim Nguyen 2J

So in irreversible processes, the tendency is for the reaction to go toward completion as quickly as possible. In the image from an older response in the link below that I found, you can see that it abruptly changes to a lower than optimal constant pressure being used in the irreversible reaction (i...

Tim Nguyen 2J

The ice cube needs energy in the form of heat to melt it further and further. By adding energy to the ice cube via the heat of your hand if you hold it, the reaction is endothermic. The ice cube absorbs the heat energy in order to melt it. An endothermic reaction is defined as a process that absorbs...

Tim Nguyen 2J

https://lavelle.chem.ucla.edu/forum/viewtopic.php?t=5062
Found this post from a while back in the forum. Hope it helps!

Tim Nguyen 2J

I think he was specifically referencing the example/problem he gave in class with the fishbowl and test tube where an exothermic reaction occurred at a constant temperature with that device in the fishbowl. There was a system where an exothermic reaction occurred inside the test tube (which is sligh...

CHEMISTRY COMMUNITY

Search found 31 matches

Re: Homework Problem 14.1

Re: Second Law application

Re: Adding OH

Re: Reaction Graphs

Re: Activation Energy

Re: Internal Energy of Isolated Systems

Re: Final Review Time Tips

Re: Internal Energy of Isolated Systems

Re: Steady State Approximation Vs Pre Equilibrium

Re: catalyst

Re: Fast or Slow

Re: -w vs +w

Re: Relationship between free energy and work

Re: 8.49

Self-Test 9.10A [ENDORSED]

Re: Entropy

Re: Midterm Topics [ENDORSED]

Re: A spontaneous reaction

Re: Heat Capacity

Re: Test question [ENDORSED]

8.113

Re: work

Re: Concepts for Chapter 8 [ENDORSED]

Re: First Law Concept

Re: 8.23

Re: 8.31

Re: 8.37

Re: Potential to do work in Irreversible vs. Reversible Expansion

Re: Endothermic Reaction

Re: Question 8.11

Re: Temperature and Exothermic Reaction [ENDORSED]