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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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1.68% is ionized

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Ka = 6.46x10⁻⁵ = [C₇H₅O₂⁻] [H₃O⁺] / [C₇H₆O₂]

<em>Where [] are concentrations in equilibrium</em>

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