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2 years ago

10

Consider this reaction: 2Al(s) + 3 CuCl2(aq) → 2AlCl3(aq) + 3 Cu(s) If the concentration of CuCl2 drops from 1.000 M to 0.655 M

in the first 30.0 s of the reaction, what is the average rate of reaction over this time interval?

2 answers:

Yuliya22 [10]2 years ago

6 0

Answer:

$r=-0.0115M/s$

Explanation:

Hello,

In this case, the rate is computed as:

$r=\frac{C_F-C_0}{T_F-T_0}$

As the reaction is analyzed during the first 30 seconds, the average rate will be:

$r=\frac{0.655M-1.000M}{30s-0s}=-0.0115M/s$

Which negative since the cupric chloride is a reagent.

Best regards.

blondinia [14]2 years ago

4 0

Answer:

rate = 0.00383 M/s

Explanation:

The rate of reaction refers to the speed at which the products are formed from the reactants in a chemical reaction

2Al(s) + 3 CuCl2(aq) → 2AlCl3(aq) + 3 Cu(s)

The equation for reaction rate in this chemical reaction (for CuCl₂) is the following one (The value 1/3 comes from the coefficient in the chemical equation for the reaction):

$\text{rate of reaction} = - \frac{1}{\text{coefficient}} \frac{Reactant}{Time}$

Here, the negative sign is used to indicate the decreasing concentration of the reactant.

$rate= -\frac{1}{3} \times \frac{C2-C1}{t2-t1}$

rate = - 1/3 [0.655 - 1.0 / 30]

rate = -1/3[-0.0115]

rate = 3.83 x 10-3 M/s

rate = 0.00383 M/s

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