# Questions tagged [rate-equation]

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### For an a plot of lnk against 1/T from Arrhenius equation, why does the y-intercept change when Ea changes?

According to Arrhenius equation, k = Ae^(-Ea/RT). Thus graph of lnk against 1/T is a straight line with negative gradient and positive y intercept. To plot a graph for lower activation energy, the ...
36 views

### Calculate concentration of product after time passed

If I have two parallel reactions: A --> P$1$ (k$_1$ = $0.00010$ s$^{-1}$) A --> P$2$ (k$_2$ = $0.00050$ s$^{-1}$) and know that the initial concentration of A is $0.0417$ M. How can I ...
25 views

### Calculating the concentration of reactants and products in parallel reactions after a time t

A substance A reacts with a solvent B to form an intermediate product IP. The reaction is bimolecular. The conc. of the solvent is constant at $12$M. IP can then react to form the two products P$1$ ...
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### Are catalyst concentrations included in the rate expression?

I have seen different rate expressions, some which include the concentration of the catalyst as a term in the rate expression, and others that do not. I thought the rate expression only includes terms ...
82 views

### Why do alkenes (olefins) burn hotter than alkanes (paraffins), even though alkanes are denser and more hydrogen-rich?

Burning hydrogen releases more total energy than combusting carbon, and all alkanes are denser as well, so why are flame temperatures for alkene molecules higher than their equivalent alkanes? P.S.: ...
23 views

### 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 ...
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### Finding the rate of a reaction given experimental data for reaction kinetics [closed]

Here is the question: For the reaction: $$\ce{2 A + 2 B → C + D}$$ The following data was obtained from three experiments: \begin{array}{c|ccc}\hline \bf{Experiment} &\textbf{[A] (mol/L)} &\...
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### Steady-state approach - how to find rate equation for intermediate?

The reaction mechanism for the formation of $\ce{NO2}$ is: \begin{align} \ce{NO + NO &<=>[$k_1$][$k_1'$] N2O2} & &\text{ (slow)} \\[0.2cm] \ce{N2O2 + O2 &->[$k_2$] NO2 +NO2} &...
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### Steady state approximation for three-step cycle

How to write the steady state for $\ce{A}?$ $$\ce{A ->[k_1] B ->[k_2] C ->[k_3] A}$$ Species $\ce{A}$ seems to appear on both side of equation as it uses itself to produce some of ...
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### Can anyone explain, why there are coefficients 2 in the equation for rate of change [A]?

The reaction mechanism for the decomposition of $\ce{A2}$ is thought to be: \begin{align} \ce{A2 &<=>[$k_1$][$k_1'$] A + A} & &\text{ (fast)} \\[0.2cm] \ce{A + B &<=>[$k_2$]...
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### Does mass affect rate of reaction?

Suppose I am reacting HCl with CuCO3. Experiment 1: I use 2g powdered CuCO3 Experiment 2: I use 4g powdered CuCO3 All other variables are kept constant. Will this have any affect on rate of reaction? ...
I am given that the enzyme concentration is $\pu{15 nM}$ and the following data: $$\begin{array}{rl} \hline S/\pu{mM} & V/\pu{mM s^{-1}} \\ \hline 1 & 0.202 \\ 2 & 0.368 \\ 5 & 0.... 1answer 73 views ### First or second order reaction I have that 100 mM of K_3Fe(CN)_6 is dissolved in equimolar of the organic ion (which I assume is HCN). In the solution Fe(CN)_6$$^{3-}$reacts to form Fe(CN)$_6^{4-}$. The formation of Fe(CN)... 1answer 111 views ### Can the RDS be different in different direction in a multi-step reversible reaction? The following mechanism is given in Peter Sykes when they are "talking about de-esterification" of an ester where the alcohol part is bulky- Here the second step is given as RDS. According ... 0answers 36 views ### Lindemann-HInshelwood mechanism difference between high and low concentration I have a gas reaction which follows the Lindemann-Hinshelwood mechanism and want to calculate the rate constant at low and at high concentrations of the gas but I find myself stuck at what my next ... 0answers 52 views ### Lindemann–Hinshelwood mechanism for a gas reaction The effective rate constant for a gaseous reaction which proceeds by a Lindemann–Hinshelwood mechanism is$\pu{1.01E-5 s^-1}$at a concentration of$\pu{4.6E-6 M}$and$\pu{2.21E-5 s^-1}$at a ... 0answers 115 views ### Effect of stirring and shaking on chemical kinetics Why don't we take the effects of stirring and shaking on the rates of chemical reactions? While studying chemical kinetics, I've seen that the rates depend on the concentrations of various species, ... 0answers 48 views ### Using the steady state approximation in the decomposition of nitramide to determine rate law$\ce{O2NNH2 (aq) ->[\mathit{k}_1] O2NNH- (aq) + H+ (aq)}\ce{O2NNH- (aq) + H+ (aq) ->[\mathit{k}_{-1}] O2NNH2 (aq)}\ce{O2NNH- (aq) ->[\mathit{k}_2] N2O(g) + OH- (aq)}\ce{H+ (aq) + OH-...
If the reaction is repeated with $\pu{2 M}$ ethyl iodide the pyridine concentration decreases as shown below. Give the rate law of the reaction in terms of pyridine and ethyl iodide. Explain your ...