All Questions
Tagged with equilibrium kinetics
115
questions
3
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1
answer
56
views
Iminium formation rate between formaldehyde and secondary amine
Given the significantly more favored hydrate of formaldehyde in the presence of water under neutral conditions, can we say that this is the slow step in iminium formation? Would removing water/working ...
- 31
3
votes
1
answer
65
views
How can a Michaelis–Menten formalism be used when enzyme concentration isn't constant?
I understand that $V_\mathrm{max} = k_3[\ce{E}]_0$ in ordinary Michaelis–Menten (MM) kinetics. According to the lecture notes provided by my university (I don't believe they are available online), ...
- 31
-1
votes
3
answers
107
views
How is it even possible that vapour pressure of liquid and vapour of solid are equal at freezing point? [duplicate]
My text book states The freezing point is defined as "the temperature at which the vapor pressure of the substance in its liquid phase is equal to its vapor pressure in the solid phase" Also ...
- 35
1
vote
1
answer
85
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Derivation of general binding equation (macromolecule with multiple binding sites)
So the last days I'm stuck at trying to solve the an equation - but I just can't (see the screenshot below.
So the idea is that you have a receptor or enzyme with multiple binding sites for a Ligand (...
- 123
0
votes
1
answer
63
views
Reaction kinetics exercise for hydrogen iodide synthesis
The rate constant for the reaction of hydrogen with iodine is $\pu{2.45E-4 M-1 s-1}$ at 302 °C and $\pu{0.905 M-1 s-1}$ at 508 °C.
a. calculate the activation energy and Arrhenius preexponential ...
- 423
2
votes
1
answer
97
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Why Michaelis Menten Assumption of equilibrium is necessary to integrate rate of ES production
I read in my textbook that the assumptions of equilibrium and of steady state used by Michaelis and Menten were simplifying assumptions intended to make the following equation one that can be ...
- 21
3
votes
0
answers
310
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Equilibrium constant of the formation of ferric thiocyanate
I was reading the paper Relaxation Kinetics of Ferric Thiocyanate (Goodall et. al, 1972) and I came across a passage which read
$\space$ Reaction (1) is the simplest representation of the equilibrium ...
- 173
3
votes
0
answers
309
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Derivation of the Van 't Hoff equation
I was reading the paper Relaxation Kinetics of Ferric Thiocyanate (Goodall et. al, 1972) and I came across the passage
Reaction (1) is the simplest representation of the equilibrium between ferric ...
- 173
0
votes
1
answer
187
views
Non-elementary reactions: Relationship between kinetic and equilibrium constant
As far as I understand, the equation for a kinetic equilibrium is always the same, and is given by:
$$K = \frac{\text{concentration of products}^{p}} {\text{concentration of reactants}^{r}}$$
Where $p$...
0
votes
0
answers
88
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Why can we use stoichiometric coefficients in the equilibrium-constant expression? [duplicate]
I just studied the chapter on chemical kinetics on Coursera, wherein I was repeatedly admonished not to use the stoichiometric coefficients in the rate law formula. I was told that this formula has to ...
- 33
-3
votes
1
answer
131
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What if kc=1 will reactants concentration equals to product concentration [closed]
I read a book, it says if kc=1 it mean reactant concentration equals to product concentration at equilibrium. But I'm wondering that in kc expression we dont just use concentration of an element we ...
- 13
2
votes
3
answers
336
views
Change of equilibrium constant with respect to temperature
Suppose we have an arbitrary chemical reaction $A+B\rightleftharpoons 2C+D$ and its equilibrium constant at two temperatures $T_{1},T_{2}$ are $k_{1},k_{2}$. We can relate them as
$$\log\frac{k_{2}}{...
- 169
1
vote
0
answers
33
views
How do metal hydrides behave in a non-hydrogen closed system?
I am curious about the fundamentals of metal hydrides and how adsorption/desorption works in non-hydrogen systems. My understanding is that the atom ratio M/Hx of the metal hydride is a function of ...
- 11
5
votes
2
answers
909
views
Effect of inert gas on the rate of reaction
Is there a general effect on the rate of reaction of a dynamic equilibrium when an inert gas is introduced at a constant volume? I know that the position of equilibrium won't change, but much like a ...
- 253
-1
votes
2
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112
views
Confused about underlying reasoning behind reaction quotient/equilibrium constant
I am a high school student taking AP Chemistry. In the unit on chemical equilibrium, there is much emphasis placed on calculating reaction quotients and equilibrium constants using this method: $$aA + ...
- 1
0
votes
0
answers
67
views
Strange behavior of equilibrium constant when most of the components are solids / pure liquids
Consider the reaction $\alpha A(g) + \beta B(s) +\gamma C(s) +\cdots \rightleftharpoons \delta D(s)+\epsilon E(s)+\cdots $, so the chemical equilibrium constant should be $\dfrac{1}{[A]^\alpha}$, ...
- 101
1
vote
0
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131
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On Le Chatelier's principle
According to my textbook,
Increasing the concentration of the reactants increases the rate of forward reaction only to reestablish equilibrium (Le Chatelier's principle)
But doesn't that also ...
- 39
3
votes
0
answers
108
views
Equilibrium concentrations of CO and Cl2 by dissociation of phosgene
I am working through a problem set from MIT's open courseware course Principles of Chemical Science.
The question is:
Phosgene $\ce{(COCl2)}$ is a chemical warfare agent that decomposes by the ...
- 49
0
votes
2
answers
100
views
chemical equilibrium and activity
Here is a graph of equilibrium coeff in various salt concentrations in water.
Lets take the example $\ce{BaSO4}$.
Now as we are increasing the salt concentration in water, the following reaction is ...
- 289
1
vote
1
answer
80
views
What is the difference between a single displacement reaction and a two competing reaction system?
For example, consider the single-displacement reaction
$$\ce{AB + C <=> BC + A}$$
My question is then if writing this reaction as the system
\begin{gather}
\ce{AB <=> A + B} \\
\ce{B + C &...
2
votes
1
answer
59
views
Rate law for thermolysis at temperatures well above the decomposition temperature
If the temperature is higher than the decomposition temperature, are thermal decomposition reactions reversible? For example, which of the following schemes would be more appropriate for temperatures ...
- 21
0
votes
0
answers
87
views
Why don't we take activities in the rate law?
I am slightly confused by the fact that concentrations and not activities are taken in the rate law which is different to equilibrium and seems to lead to a discrepancy. For example, for the reaction $...
- 92
0
votes
1
answer
58
views
Are there any well documented reactions with "persistent" intermediates
I'm a biology and/or math person, not a chemistry person. I have only taken the standard sequence of undergraduate courses up to organic chemistry, and that was some time ago, so please excuse (and ...
- 101
2
votes
1
answer
459
views
Combining two reactions in equilibrium with same reactants but different products: What would be the new K?
If I have the reactions :
A(g) ⇌ B(g) K1
A(g) ⇌ C(g) K2
Am I able to add the equations like done in Hess's law despite nothing canceling out? And if I can do so, is the new equilibrium ...
- 41
0
votes
1
answer
1k
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How to relate equilibrium constant and equilibrium conversion?
For the following gas phase reaction:
$$ A\leftrightarrow B $$
The concentration equilibrium constant ($K_c$) can be expressed as:
$$ K_c = \frac{c_B}{c_A} = \frac{\frac{F_B}{\vartheta}}{\frac{F_A}{\...
- 17
1
vote
1
answer
314
views
How does the rate equation account for solids and liquids?
The question is long because I wanted to include the whole thought process.
Given the hypothetical reaction:
$$\ce{ A(s) + B(aq) <=> C(aq) + D(aq)}$$
One would obtain the equilibrium constant:
$$...
- 360
2
votes
0
answers
41
views
Do decomposition potentials change during electrolysis?
I was just wondering if decomposition potentials actually change during electrolysis. For example, if we reversed the Daniell cell reaction so that copper is oxidized, the half cell reactions would be:...
user115162
8
votes
4
answers
833
views
Deriving kinetic equations for reversible reactions
Problem
Given the reaction $\ce{A <=>[$k_\mathrm f$][$k_\mathrm b$] B}$ with rate constants $k_\mathrm f = \pu{4E-2 s-1}$ and $k_\mathrm b = \pu{10^{-2} s-1}$. Initially, $\pu{2 mol}$ of $\ce{A}...
- 1,817
0
votes
1
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119
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How is the equilibrium expression (law of mass action) related to the rate law? [duplicate]
Every chemistry textbook I've read will have a chapter on the rate law. It will say something like, given a reaction $a\text{A} + b\text{B} \rightarrow c\text{C} + d\text{D}$, the rate law (for the ...
- 11
0
votes
0
answers
24
views
Why is the concentration of gases denoted in form of partial pressure? [duplicate]
In most of the chemical laws of chemistry involving concentration of products or reactants like equilibrium constant, reaction quotient, Henry's law, Nernst equation etc, I often see a similar note ...
user112102