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Why rate constant decrease when activation increase in arrhenius equation?
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Does the temperature have to be in Kelvin for the Arrhenius equation?
Yes, since the R constant has units of Latm/molK, temperature must be in K
Who created the Arrhenius equation?
The Arrhenius equation was created by Svante Arrhenius in 1889, based on the work of Dutch chemist J. H. van't Hoff. The rate equation shows the effect of changing the concentrations of the reactants on the rate of the reaction.
How would cooling down a solution change reaction time?
In general, cooling a solution slows the reaction. You can use the Arrhenius equation to figure out what effect a given temperature will have on a particular reaction (you'll need to know the activation energy).
Does an increase in pressure at constant temperature increase the rate constant of a reversible reaction in both directions?
The rate constant is unaffected, as demonstrated by Arrhenius equation: k = Ae^(-E/RT) where A is the pre-exponential factor (constant for a particular reaction) E is the activation energy R is the molar gas constant T is the thermodynamic temperature However, when pressure is increased at constant temperature for a gaseous reversible reaction, the concentrations of every reactant and product increase by the SAME factor. Since Kp (pressure equilibrium constant) is to remain constant, it means that the position of equilibrium will shift in such a way so as to decrease the total number of moles of gaseous species. Note: This answer can be improved by proving the last statement using a general example which, due to lack of time, I skipped. (Although some people might get the logic!!!)
How do you calculate energy of activation in catalysis?
This is to be calculated from at least two identical kinetic experiments1) only varying the temperature. Use the Arrhenius equation2):kT = A * e^[-Ea/R.T ]in which: (all in SI units: J, mole, K as applicable) kT = rate constant, measured at temp. T1 or T2A = Arrhenius factor, (largely) independent of temperature (if |T1-T2| < 25 K)e^ = power of e, e being the base of the natural logarithm, e=2.71828...Ea = activation energy of the particular reaction (independent of temperature and concentration)R = universal gas constantT = temperature (T1 or T2, both > 250 K)1) All reaction parameters should be the same except temperature.2)The Arrhenius equation is a simple, but remarkably accurate, formula for the temperature dependence of the rate constant, and therefore, rate of a chemical reaction.The equation was first proposed by the Dutch chemist J. H. van 't Hoff (who was my 'chemical grandfather' when I was 14, at my first chemical college) in 1884; five years later in 1889, the Swedish chemist Svante Arrhenius provided a physical justification and interpretation for it.
Will affect the rate of the constant according to the Arrhenius equation changing which factors?
Temperature and activation energy
According to the Arrhenius equation changing which factors will affect the rate constant?
Temperature and activation energy - apex
How does activation energy affect chemical reactions?
The Arrhenius equation is: Ea = -RT ln(k/A) where Ea - activation energy R - universal gas constant ln - logarithm k - speed constant T - temperature in kelvins
What is the Arrhenius equation?
It is an equation that relates the speed at which a chemical reaction progresses with the activation energy and the temperature of the reactants and products. k = A * e^(-Ea/(R*T)) Where k = velocity constant (different for each reaction) A = pre-exponential factor Ea = activation energy R = universal gas constant (=8,314J/molK) T = temperature
What is an Arrhenius equation?
An Arrhenius equation is an equation which approximates the dependence of the rate of any chemical reaction on the temperature.
If HCL and Na2S2O3 are kept constant by how many degrees would this reaction have to be heated from 25 degrees C to precisely double the reaction rate?
You need to use the Arrhenius equation to solve this kind of problem. Since you haven't given the activation energy, we can't answer it for you.
Does the temperature have to be in Kelvin for the Arrhenius equation?
Yes, since the R constant has units of Latm/molK, temperature must be in K
What is the connection between accelerated aging test of a material and Arrhenius equation?
The Arrhenius equation is a formula for the dependence of reaction rates on temperature. The accelerated aging test of a material depends on the Arrhenius equation for it to work.
Who created the Arrhenius equation?
The Arrhenius equation was created by Svante Arrhenius in 1889, based on the work of Dutch chemist J. H. van't Hoff. The rate equation shows the effect of changing the concentrations of the reactants on the rate of the reaction.
How do you determine Ea by Arrhenius equation?
yes
Is rate constant equal to one over TIME in the Arrhenius Equation If so or not is there an equation representing their relationship?
The unit of the rate constant in a 1st Order reaction rate equation (NOT the 'Arrhenius equation', as stated in the question) is One over Time.General form of a reaction rate equation :rate (mol.L-1.time-1) = [rate constant(Ln-1.mol1-n.time-1)]*[Concentration()]nwhere:* n is the Order of the rate equation (that is of the rate limiting step) * all units are (italicalised) between brackets It can easily be seen in this that for n=1 (1st Order) the equation is:r = k * C1and in units:mol.L-1.time-1 = (L0.mol0.time-1)*(mol.L-1)1so:(mol.L-1.time-1) = (time-1)*(mol.L-1)Only the value of the rate constant k is depending on temperature only (cf. Arrhenius equation), though temperature is NOT in its unit.
How would cooling down a solution change reaction time?
In general, cooling a solution slows the reaction. You can use the Arrhenius equation to figure out what effect a given temperature will have on a particular reaction (you'll need to know the activation energy).
