Problem: For the reaction given, the FeCl3 changes from 1.000 M to 0.444 M in the first 10 seconds.Calculate the average rate in the first 10 seconds. 2 FeCl3 (s) → 2 Fe (s) + 3 Cl2 (g) a. 0.0384 M/sb. 0.210 M/sc. 0.0278 M/sd. 0.0874 M/se. 0.568 M/s 

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FREE Expert Solution
FREE Expert Solution

We’re being asked to calculate the average rate of the reaction for the following reaction:

2 FeCl3(s)  2 Fe(s) + 3 Cl2(g)


For the reaction, the concentration FeCl3 changes from 1.000 M to 0.444 M in the first 10 seconds.



Recall that for a reaction aA  bB, the rate of a reaction is given by:


Rate=-1aΔ[A]Δt=1bΔ[B]Δt


where: 

Δ[A] = change in concentration of reactants or products (in mol/L or M), [A]final – [A]initial

Δt = change in time, tfinal – tinitial


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Problem Details

For the reaction given, the FeCl3 changes from 1.000 M to 0.444 M in the first 10 seconds.

Calculate the average rate in the first 10 seconds. 

2 FeCl3 (s) → 2 Fe (s) + 3 Cl2 (g) 

a. 0.0384 M/s

b. 0.210 M/s

c. 0.0278 M/s

d. 0.0874 M/s

e. 0.568 M/s 

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Based on our data, we think this problem is relevant for Professor Young's class at ST THOMAS.