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

For the reaction given, the FeCl_{3} changes from 1.000 M to 0.444 M in the first 10 seconds.

Calculate the average rate in the first 10 seconds.

2 FeCl_{3} (s) → 2 Fe (s) + 3 Cl_{2} (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

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

2 FeCl_{3}(s) → 2 Fe(s) + 3 Cl_{2}(g)

For the reaction, the concentration FeCl_{3} 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:

$\overline{){\mathbf{Rate}}{\mathbf{=}}{\mathbf{-}}\frac{\mathbf{1}}{\mathbf{a}}\frac{\mathbf{\Delta}\mathbf{\left[}\mathbf{A}\mathbf{\right]}}{\mathbf{\Delta t}}{\mathbf{=}}\frac{\mathbf{1}}{\mathbf{b}}\frac{\mathbf{\Delta}\mathbf{\left[}\mathbf{B}\mathbf{\right]}}{\mathbf{\Delta t}}}$

where:

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

**Δt** = change in time, *t _{final} – t_{initial}*

Average Rate of Reaction

Average Rate of Reaction

Average Rate of Reaction

Average Rate of Reaction