CHEMISTRY COMMUNITY

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Calculate the activation energy, Ea , in kilojoules per mole for a reaction at 65.0 C that has a rate constant of 0.238 s^−1 and a frequency factor of 2.09×1011 s^−1 .

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catalysts do not affect the concentration of the reactants nor products. They only affect activation energy.

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First- order: t1/2 = ln (2) / k

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I believe that both equations are just different versions of each other, but produce the same values.

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If the molecule is used at the beginning of a reaction and later preproduced at the end of the reaction it is the catalyst.

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nitrogen has an oxidation state of -2

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as t refers to time it does not matter whether you choose sec, min, or h as long as you match it up with the rest of the problem

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I would say doing syllabus textbook problems and going through some achieve problems.

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yes, it is cumulative. Final is 13th

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It is going to be the same structure as the previous exams

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It just means knowing how to implement the ideal gas law equation into a problem.

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Anderson library is really nice

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Look at the units in the question and use the according R value

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second order reaction will be a positive linear line on a graph with the y axis as 1/[A] and the x axis as time.

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rate=k[I−][ClO−]/[OH−]

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I am still confused on part 5. Would it be [17]^2 [100]^2 [280]??

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Zero Order: k = M/s

First Order: k = 1/s

Second Order: k = 1/(M*s)

Third Order: Rate = k= 1/(M^2*s)

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A simple way to determine this is by looking at the graphs of the reaction. Understanding the reaction order graph trends will allow you to determine the order of the reaction.

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it is a chemical reaction in which the rate of reaction is directly proportional to the concentration of the reacting substance. This reaction depends linearly on only one reactant concentration.

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There are a set of oxidation number rules. I would just suggest that you do practice problems so it is ingrained in your mind. But besides that, Oxygen usually has a -2 oxidation number, unless it is in a peroxide, in which case it is -1. Hydrogen is usually +1. With those two, you can usually figur...

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You should probably know how to derive equations. Just know the basic concepts and when/how to implement the equations.

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We will be taking the exam the same exact way as we have been for the midterms.

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Think of k as the equilibrium constant and k as the rate constant.

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Kinetic control: A reaction in which the product ratio is determined by the rate at which the products are formed. Thermodynamic control: A reaction in which the product ratio is determined by the relative stability of the products. One has more kinetic product and the other has more thermodynamic p...

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You can tell if it’s oxidized or reduced based off the elements oxidation number from the reactant side. If the charge decreases on the product side, then it’s being reduced. If the charge alters to agreateer number, it is being oxidized.

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The zero and second order reactions are dependent on K because their equations include [A]o as a term.
The half life of first order reactions is independent of [A]o given the equation 0.693/k.

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catalysts decrease the activation energy for the reaction in both the forward and reverse.

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Do not get it mixed up with catalysts which only increase the rate of a chemical reaction and do not get consumed (they appear in reactants and product side). Intermediates get consumed in a reaction, so they appear as products but subsequently get used up as reactants.

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Free expansion is an irreversible process in thermodynamics in which a volume of gas is kept in one side of a thermally isolated container (via a small partition), with the other side of the container being evacuated.

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Balancing equations in a basic solution uses OH-, while an acidic solution you can use H+. Reactions with H+ can always be converted to basic (using OH-) by adding water and balancing it out.

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Under conditions that the system is at constant pressure and no expansion work is being done on the system, the q and delta H values are equivalent.

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This equation sums up the heat of the system with work being done on or by the system which is -P * change in volume.

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How do I determine which R value to use?

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I agree, any form works and make sure to pay attention to what the questions asks of you (J, kJ).

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How do we determine if the reaction is spont or nonspont?

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what does the standard potential of a cell mean in terms of context?

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Identify the oxidizing and reducing agents in the skeletal (unbalanced) reaction. Then, balance the reaction, including the phase (solid, liquid, etc.) of each species. The reaction takes place in basic aqueous solution. N2H4(g)+ClO−3(aq)⟶NO(g)+Cl−(aq) I am still not sure how to make the balanced eq...

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How do we determine what a 2nd order reaction line looks like?

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How do we know what the curve of first order reaction looks like?

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How do we determine what the curve of the zero order graph looks like?

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happy valentines

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The presence of a catalyst provides a reaction pathway in which the activation energy of a reaction is reduced by 42.00 kJ⋅mol−1 . Uncatalyzed: A⟶B Ea=128.00 kJ⋅mol−1 Catalyzed: A⟶B Ea=86.00 kJ⋅mol−1 Determine the factor by which the catalyzed reaction is faster than the uncatalyzed reaction at 295....

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Catalysts speeds up a chemical reaction, or lowers the temperature or pressure needed to start one, without itself being consumed during the reaction

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How do you determine which species is a catalyst?

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How do I find the detailed answer key for the textbook?

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For the reversible, one‑step reaction, A+A⥫⥬=k−1k1B+C the rate constant for the forward reaction, k1 , is 287 L⋅mol−1⋅min−1 and the rate constant for the reverse reaction, k1 , is 359 L⋅mol−1⋅min−1 at a given temperature. The activation energy for the forward reaction is 44.7 kJ⋅mol−1 , whereas the ...

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A certain reaction has an activation energy of 69.64 kJ/mol. At what Kelvin temperature will the reaction proceed 4.00 times faster than it did at 343 K?

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The mechanism proposed for the oxidation of iodide ion, I−, by the hypochlorite ion, ClO−, in aqueous solution is shown. ClO−(aq)+H2O(l)⇌HClO(aq)+OH−(aq)fast in both directions I−(aq)+HClO(aq)→HIO(aq)+Cl−(aq) slow HIO(aq)+OH−(aq)→IO−(aq)+H2O(l) fast Complete the rate law for the formation of IO− imp...

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A particular reactant decomposes with a half‑life of 161 s when its initial concentration is 0.343 M. The same reactant decomposes with a half‑life of 245 s when its initial concentration is 0.225 M.
Determine the reaction order.

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The rate of the given reaction is 0.480 M/s.
A+3B⟶2C

What is the relative rate of change of each species in the reaction?

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You would use mass if you have the specific heat capacity and if you have the molar heat capacity, use moles (n)

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You would use mass if you have the specific heat capacity and if you have the molar heat capacity, use moles (n)

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Remember that reduction is if electrons are being gained, resulting in a gain of negative charge. In oxidation, the charge gets more positive.

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