Constants  Periodic Table Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table:

Part a Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units. View Available Hint(s)
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Part 1)
Here, rate = k[A]^{2} [B]
From experiment (1)
1.5 x 10^{2} = k x 0.5^{2} x 0.05
Therefore, k= (1.5 x 10^{2}) / (0.5^{2} x 0.05) = 1.2 M^{2}s^{1}
Now, initial rate for the formation of C at 25 ^{∘}C, if [A] = 0.50M and [B] = 0.075M can be calculated as,
Rate = 1.2 x [0.5]^{2} x [0.075] = 0.022 M/s
Part 2)
Rate of formation of P_{2}O_{5} = −Δ[A]/Δt = [(8.90×10^{−3})( 2.90×10^{−3})] / (4010)
= (6 × 10^{−3}) / 30 = 2 x 10^{4} M/s
Part 3)
Here, this part is incomplete, the average rate of consumption of Br^{} is not provided.
If you know the average rate of consumption of Br^{}, then according to the following reaction,
5Br^{}(aq) + BrO_{3}^{}(aq) + 6H^{+}(aq) → 3Br_{2}(aq) + 3H_{2}O (l)
Average rate of consumption of H^{+} = average rate of consumption of Br^{} x (6/5)
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