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If a temperature increase from 22.0 to 34.0 triples the rate constant for a reaction what is the value of the activation barrier for the reaction?
Wiki User
∙ 11y ago
69.0kJ/mol
Wiki User
∙ 11y ago
Wiki User
∙ 11y ago69.0 kJ/mol
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Can a reaction have zero activation energy?
if a reaction is carried out at constant temperature to completion it will have a zero activation energy.
How do changes in temperature and energy influence chemical changes?
The reaction rate is dependent on temperature (increasing the temperature the reaction rate increase) and activation energy.
What happens to the rate constant of a chemical reaction when the temperature increases?
Increasing the temperature will cause there to be an increase in kinetic energy. This results in an increase in collision frequency, and eventually an increase in rate of reaction as well.
How do changes in temperature and activation energy compare in how they affect reaction rate Apex?
Changes in temperature and activation energy have opposite effects on reaction rate.
If the temperature of a reaction increases what happens to the value of the equilibruim constant?
Equilibrium constant changes when temperature changes. For an endothermic reaction, the equilibrium constant increases with temperature while for an exothermic reaction equilibrium constant decreases with increase in temperature. Equilibrium constants are only affected by change in temperature.
Can a reaction have zero activation energy?
if a reaction is carried out at constant temperature to completion it will have a zero activation energy.
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
How do changes in temperature and energy influence chemical changes?
The reaction rate is dependent on temperature (increasing the temperature the reaction rate increase) and activation energy.
How do changes in energy and temperature influence chemical changes?
The reaction rate is dependent on temperature (increasing the temperature the reaction rate increase) and activation energy.
How an increase in temperature change the rate constant of a chemical reaction?
yes ofcourse!
What happens to the rate constant of a chemical reaction when the temperature increases?
Increasing the temperature will cause there to be an increase in kinetic energy. This results in an increase in collision frequency, and eventually an increase in rate of reaction as well.
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
How do changed in temperature and activation energy compare in how they affect reaction rate?
Changes in temperature and activation energy have opposite effects on reaction rate.
How do changes in temperature and activation energy compare in how they affect reaction rate Apex?
Changes in temperature and activation energy have opposite effects on reaction rate.
If the temperature of a reaction increases what happens to the value of the equilibruim constant?
Equilibrium constant changes when temperature changes. For an endothermic reaction, the equilibrium constant increases with temperature while for an exothermic reaction equilibrium constant decreases with increase in temperature. Equilibrium constants are only affected by change in temperature.
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!!!)
Why does increasing the temperature of a reaction increase its rate?
It provides energy to overcome the activation energy.
