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zaharov [31]
3 years ago
10

In the first 21.0 s of this reaction, the concentration of HBr dropped from 0.550 M to 0.506 M . Calculate the average rate of t

he reaction in this time interval.
Chemistry
1 answer:
timofeeve [1]3 years ago
8 0

Answer:

1.048x10⁻³M/s is the rate of reaction

Explanation:

Based on the reaction:

2HBr → H₂ + Br₂

The rate of reaction is defined as:

1/2 Δ[HBr] / Δt

<em>1/2 because the reaction is consuming 2 times HBr per mole of reaction</em>

<em>Where </em>Δ[HBr] is 0.550M - 0.506M = 0.044M

And Δt is 21.0s. The average rate of reaction is:

1/2 0.044M / 21.0s =

<h3>1.048x10⁻³M/s is the rate of reaction</h3>
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Explanation:

When there are more number of hydroxide ions in a solution then there will be high concentration of OH^{-} or hydroxide ions. As a result, more will be the strength of base in that particular solution.

A base is strong when it readily dissociate into its ions in the solution. When a base is strong, then it does not matter at what concentration it is dissolved in the solution because despite of its low concentration it will remain a strong base.

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Answer:

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Explanation:

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