Question

Calculate the rate at which \( B \) and \( C \) are formed if \( A \) is consumed at \( 3.6 \times 10^{-4} \mathrm{M} / \mathrm{s} \) \[ 2 A \rightarrow 4 B+C \]

          Calculate the rate at which \( B \) and \( C \) are formed if \( A \) is consumed at \( 3.6 \times 10^{-4} \mathrm{M} / \mathrm{s} \)
\[
2 A \rightarrow 4 B+C
\]

Calculate the rate at which B and C are formed if A is consumed at 3.6 × 10^-4M / s

2 A → 4 B+C

Added by Jennifer A.

Chemistry The Science in Context

Thomas R. Gilbert 5th Edition

Chapter 13

Instant Answer

Solved by Expert David Collins

09/02/2020

Step 1

For every 2 moles of A consumed, 4 moles of B and 1 mole of C are produced. So, if the rate of consumption of A is 3.6 x 10^-4 M/s, then the rate of formation of B is twice that, because for every 2 moles of A consumed, 4 moles of B are produced. Show more…

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