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30 Cards in this Set
- Front
- Back
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the study of the rate of chemical reactions |
chemical kinetics |
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change in molar concentration of the reactant or product with time |
rate of reaction |
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rate of reaction formula |
rate = - ∆[R] / ∆t |
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rate of product formula |
rate = ∆[P] / ∆t |
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series of steps by which reactants are converted into products called |
reaction mechanism |
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reaction to occur molecules atoms or ions must collide effectively |
collision theory |
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end of reactants; state of reactants |
nature of the reactants |
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high temperature accelerates rate of reaction |
temperature |
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high concentration, the faster the rate of reaction |
concentration |
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greater surface area has faster rate of reaction |
surface area |
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lowers the activation energy |
catalyst |
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amount of kinetic energy that particles must process in order to react |
activation energy |
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that increases the rate of chemical reaction without being used up in the reaction by lowering the activation energy |
catalyst |
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mathematical statement expression which relates the reaction rate to the concentration of the reactant raised to a certain exponent or power |
rate equation or rate law |
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rate law expression |
Rate = k[R]^x |
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indication of how fast or slow is the rate of reactinon. the higher the value of k the faster the rate of reaction |
rate constant (k) |
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proportional to molar concentration of reactant what order of reaction |
first order [R]¹ |
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order of reaction where the reaction rate varies directly to the square of molar concentration of the reactant |
second order reactant [R]² |
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the reaction rate does not depend on the molar concentration of the reactant which order of the reactant |
zero order reactant [R]⁰ |
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reactions that do not go to completion and that can occur in either direction are called |
reversible reaction |
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when a reversible reaction has a tape equilibrium at a given temperature the product of the molar concentration of the product divided by the product the motor concentration of the reactants with each concentration raised to the power equal to the coefficient in the balanced equation is a constant |
law of mass action |
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species in a single phase |
homogeneous equilibrium |
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species in more than one phase |
heterogenous equilibrium |
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measure of the extent to which a reaction occurs |
magnitude of Keq |
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reaction must offer to a greater extent than the reverse reaction for equilibrium to be established |
Q<Keq |
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reverse reaction must occur to agree the extent than the forward reaction for equilibrium to be established |
Q>Keq |
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the system is already in equilibrium so now for the net reaction occurs |
Q=Keq |
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ph1-6 |
acid |
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ph 0 |
neutral |
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ph 7-8 |
base |
