Reaction: A --> B Expression: Rate = k[A] Using this expression, determine the Rate when: k = 0.000396 s-1 [A] = 0.0508 mol L-1
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The rate of the reaction is expressed as: \[ \text{Rate} = k[A] \] Show more…
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For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.10 0.10 0.10 3.0×10−5 2 0.10 0.10 0.30 9.0×10−5 3 0.20 0.10 0.10 1.2×10−4 4 0.20 0.20 0.10 1.2×10−4 k = 3.0×10−2 M−2⋅s−1 Order of reaction for A=2 Order of reaction for B=0 Order of reaction for C=1 Given the data calculated in Parts A, B, C, and D, determine the initial rate for a reaction that starts with 0.45 M of reagent A and 0.70 M of reagents B and C? Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.
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The rate constant of a first-order reaction: $\mathrm{A} \longrightarrow$ products, is $60 \times 10^{-4} \mathrm{~s}^{-1} .$ Its rate at $[\mathrm{A}]=$ $0.01 \mathrm{~mol} \mathrm{~L}^{-1}$ would be (a) $60 \times 10^{-6} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$ (b) $36 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$ (c) $60 \times 10^{-2} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$ (d) $36 \times 10^{-1} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~min}^{-1}$
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