# Questions tagged [rate-equation]

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### Calculating ionic strength at different concentrations

Zn$^{2+}$ reacts with a molecule, B, in a solution at several different concentrations of NaCl. Determine the charge of the biomolecule and k$_0$ (second order) ​​(assume that Zn$^{2+}$ does not ...
• 721
Below are four reactions, to this experiment inhibitor is added so that k$_3$ = $0$ (but the other reactions are unaffected) calculate [D] when the reaction is over. The initial concentration of A is $... • 721 -1 votes 1 answer 225 views ### Why is it that first order reactions never end? [duplicate] I'm studying chemical kinetics in high school. We are studying Integrated Rate Equation of first order reactions - their derivations and graphs. Our teacher showed us a graph of: Concentration of ... 1 vote 1 answer 60 views ### How to calculate rate of carbon dioxide from rate equation? [closed] The concentration of carbon dioxide that changes with time: $$\ce{CO2(g) + H2O(l) <=>[k_\mathrm{fwd}][k_\mathrm{rev}] HCO3-(aq) + H+(aq)}$$ How to calculate the integral for the following ... • 11 0 votes 0 answers 23 views ### Can two 1st order reactants in an overall 2nd order reaction have different rates? I've recently done a saponification reaction of ethyl acetate with sodium hydroxide and used the initial rates method to find the order of reaction. (I change the concentration of one reactant and ... • 27 -1 votes 1 answer 52 views ### Rate equation for the decomposition of hydrogen peroxide with iron(III) chloride as catalyst [duplicate] I am trying to determine the activation energy of the decomposition of hydrogen peroxide with iron(III) chloride added as a catalyst. To do that, I need to find the rate constant, but I am not sure ... 3 votes 2 answers 162 views ### Does 'k' in the rate law change with a change in volume I'm a high school AP Chem student and we recently learned about the rate law and the Arrhenius equation. In school, we learned that rate constant 'k' is only changed with temperature or catalyst. ... • 103 0 votes 0 answers 25 views ### How can gradient of concentration-time graph be zero at equlibirum if the rate of reaction is non zero? The rate of a reaction is usually measured as the rate of change of the concentration of a reactant or product with respect to time. Also, at equilibrium, the rates of the forwards and reverse ... -1 votes 1 answer 118 views ### Rate of Reaction - Potassium Permanganate and Hydrogen Peroxide I'm interested in an aerospace project that requires I know the reaction rate ($[\pu{M/s}]) of, $$\ce{2 KMnO4 (aq) + 3 H2O2 (aq) -> 3 O2 (g) + 2 MnO2 (s) + 2 KOH (aq) + 2H2O (l)}.$$ I'm just ... 9 votes 1 answer 250 views ### Are there any genuine, elementary ternary reactions? Macroscopically, reaction rates can be of varied order. But mechanistically, most reactions are first-order or second-order/binary (e.g. SN2, many catalyst surface reactions, dimers). Most processes ... • 251 -1 votes 1 answer 140 views ### Writing rate of disappearance and rate of appearance using rate law [closed] I have studied that rate of disappearance and rate of appearance is the change in concentration of reactants and products (respectively) with respect to time. Thus, $$\text{ROD} = -\frac{\Delta c_R}{\... • 137 0 votes 0 answers 246 views ### Assuming 2O3 (g) → 3O2 (g), how much oxygen will be formed within 5.50 s for a reaction rate of 0.250 M/s? Context: The rate of appearance of \ce{O2} in the reaction: \ce{2O3 (g) -> 3O2 (g)} is \pu{0.250 M/s}. So, over the first \pu{5.50 s}, will it form \pu{1.38 M}, or \pu{4.13 M} of oxygen ... -1 votes 2 answers 641 views ### What is the rate law of a reaction: 2A + 3B → products? [closed] Update: I found out that the coefficients of the chemical reaction are not the exponents in the rate law. It is actually the order of the species during the reaction. It is known that in the reaction, ... 0 votes 1 answer 61 views ### Problem understanding the rate of reaction of reversible reactions Case 1:$$\ce{CH_3COOH + NaOH<=>CH_3COONa + H_2O}$$At equilibrium, there remain extremely small concentrations of the reactants (acetic acid and sodium hydroxide), and comparatively large ... • 23 3 votes 0 answers 29 views ### The Mechanism of Termolecular Reactions How does a termolecular elementary reaction happen under the law of mass action? My physical chemistry textbook only says details about bimolecular and unimolecular reactions with collision theory. I ... • 31 0 votes 1 answer 190 views ### Can an elementary reaction have zero order? I am very confused right now about my approach to this question could somebody help me out with this. I reasoned my answer as given below Let's assume if a complex reaction is of zero order. It ... 0 votes 1 answer 86 views ### Calculate concentration of product after time passed If I have two parallel reactions: A --> P1 (k_1 = 0.00010 s^{-1}) A --> P2 (k_2 = 0.00050 s^{-1}) and know that the initial concentration of A is 0.0417 M. How can I ... • 721 0 votes 0 answers 43 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 12M. IP can then react to form the two products P1 ... • 427 1 vote 0 answers 88 views ### Determining reaction order from absorbance A reaction is initiated in a solution which contained a dissolved component. The transmittance was measured at \pu{240 nm} in a \pu{2.54 cm} long cell. At t = 0 the transmittance was 1. \... • 721 0 votes 0 answers 48 views ### Determining ion charge using rate constants and ionic strength I am given the following data: The rate constant k at \pu{25 ^\circ C} in a reaction of persulfate ions and iodide ions in a water solution is assumed to vary with the total ionic strength of the ... • 721 8 votes 4 answers 278 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}... • 1,773 0 votes 0 answers 45 views ### 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 ... 5 votes 2 answers 219 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.: ... • 1,659 0 votes 1 answer 39 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 ... • 11 2 votes 1 answer 80 views ### 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)} &\... • 31 5 votes 2 answers 108 views ### 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} &... • 71 3 votes 0 answers 63 views ### 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 ... • 31 4 votes 1 answer 182 views ### 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]... • 49 0 votes 1 answer 907 views ### 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? ... • 3 4 votes 2 answers 743 views ### Determine vmax and enzyme concentration (Michaelis–Menten) 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.... • 427 3 votes 1 answer 95 views ### First or second order reaction I have that100$mM of K$_3$Fe(CN)$_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-}$. The formation of Fe(CN)... • 427 3 votes 1 answer 160 views ### Can the RDS be different in different direction in a multi-step reversible reaction? The following mechanism is given in Peter Sykes when they are "talking about de-esterification" of an ester where the alcohol part is bulky- Here the second step is given as RDS. According ... • 353 2 votes 0 answers 49 views ### Lindemann-HInshelwood mechanism difference between high and low concentration I have a gas reaction which follows the Lindemann-Hinshelwood mechanism and want to calculate the rate constant at low and at high concentrations of the gas but I find myself stuck at what my next ... • 427 4 votes 0 answers 87 views ### Lindemann–Hinshelwood mechanism for a gas reaction The effective rate constant for a gaseous reaction which proceeds by a Lindemann–Hinshelwood mechanism is$\pu{1.01E-5 s^-1}$at a concentration of$\pu{4.6E-6 M}$and$\pu{2.21E-5 s^-1}$at a ... • 427 2 votes 0 answers 394 views ### Effect of stirring and shaking on chemical kinetics Why don't we take the effects of stirring and shaking on the rates of chemical reactions? While studying chemical kinetics, I've seen that the rates depend on the concentrations of various species, ... • 1,308 1 vote 0 answers 65 views ### Using the steady state approximation in the decomposition of nitramide to determine rate law$\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 ...