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For the following reaction, the rate law...

For the following reaction, the rate law has been determined to be Rate = `k[A][B]^2" with " k = 2.0 xx 10^(-6) mol^(-2) s^(-1)`
`2A + B C to A_2B + C`
Determine the rate after 0.06 mol `L^(–1)` of A has reacted.

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To determine the rate of the reaction after 0.06 mol L^(-1) of A has reacted, we will follow these steps: ### Step 1: Write down the rate law The rate law for the reaction is given as: \[ \text{Rate} = k[A][B]^2 \] where \( k = 2.0 \times 10^{-6} \, \text{mol}^{-2} \, \text{s}^{-1} \). ### Step 2: Determine the initial concentrations of A and B ...
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