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igomit [66]
3 years ago
14

For the second-order reaction below, the initial concentration of reactant A is 0.24 M. If the rate constant for the reaction is

1.5 x10–2 M–1s–1, what is the concentration of A after 265 seconds?2A --> B + Crate = k[A]20.12 M0.19 M0.95 M4.0 M5.2 M
Chemistry
1 answer:
CaHeK987 [17]3 years ago
7 0

Answer:

Concentration of A after 265 seconds is 0.12 M

Explanation:

Integrated rate law for the given second order reaction is-

                            \frac{1}{[A]}=\frac{1}{[A]_{0}}+kt

where [A] is concentration of A after "t" time, [A]_{0} is intital concentration of A and k is rate constant.

Here [A]_{0} is 0.24 M, k is 0.015 M^{-1}S^{-1} and t is 265 S

Plug in all the values in the above equation-

                               \frac{1}{[A]}=\frac{1}{0.24}+(0.015\times 265)

                              or, [A] = 0.12

So concentration of A after 265 seconds is 0.12 M

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Let's consider the following balanced reaction.

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We can calculate the standard enthalpy change for the reaction (ΔH°r) using the following expression.

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A 4.24 kg marble slab has the volume of 1564 cm3 What is the density in g/cm3
miskamm [114]

Answer:

The answer is

<h2>2.71 g/cm³</h2>

Explanation:

The density of a substance can be found by using the formula

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