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Irina18 [472]
3 years ago
10

The rate of reaction in terms of the "rate law expression" includes the rate constant (k), the concentration of the reactants, a

nd the orders of the reaction with respect to the different reactants. Consider the following reaction: A+B→C+D The initial concentrations of the reactants A and B are 0.400 M and 0.290 M, respectively. The rate of reaction is 0.060 M⋅s−1, and the orders of the reaction, with respect to reactants A and B, are 1 and 2, respectively. Determine the rate constant (k) for the reaction using the rate law. Express your answer in M−2⋅s−1 to three significant figures. View Available Hint(s) The rate constant(k) k (k) = nothing M−2⋅s−1
Chemistry
1 answer:
Ainat [17]3 years ago
8 0

Answer:

1.78 M⁻²s⁻¹

Explanation:

Let's consider the following reaction:

A + B → C + D

The reaction order for A is 1 and the reaction order for B is 2.

The rate law is:

r = k.[A].[B]²

where,

r is the rate of the reaction

k is the rate constant

[A] and [B] are the molar concentrations of the reactants

Then, we can find the value of k.

r=k.[A].[B]^{2} \\k=\frac{r}{[A].[B]^{2} } =\frac{0.060M.s^{-1} }{(0.400M).(0.290M)^{2} } =1.78M^{-2} s^{-1}

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You will want to find how many grams are in a whole mole so you know which element it is. To do this, find out how much of a mole you have.

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Now we know that, find what to multiply 20 g by to get the rest of the mole.

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Answer : The time passed in years is 2.74\times 10^2\text{ years}

Explanation :

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First we have to calculate the rate constant, we use the formula :

k=\frac{0.693}{t_{1/2}}

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Expression for rate law for first order kinetics is given by:

t=\frac{2.303}{k}\log\frac{a}{a-x}

where,

k = rate constant  = 1.21\times 10^{-4}\text{ years}^{-1}

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Now put all the given values in above equation, we get

t=\frac{2.303}{1.21\times 10^{-4}}\log\frac{15.3}{14.8}

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A reaction is referred to as a redox reaction if two or more reactants belonging to a single reaction exchange one or more electrons, i.e., one reactant releases one or more additional electrons while the other obtains one or additional electrons. The reacted substance that releases electrons is oxidized and becomes a reducing substance. A reduced oxidizing agent is the reactant that accepts electrons.

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