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Consider the following reaction at 277 K: A + 2B â C + D where rate = k[A][B]2. An experiment was performed where [A]o = 0.00205 M and [B]o = 2.55 M. A plot of ln[A] vs. time has a slope of -10.31. What will the rate of this reaction be when [A] = [B] = 0.371 M?

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Consider the following reaction at 277 K: A + 2B â C + D where rate = k[A][B]2. An experiment was performed where [A]o = 0.00205 M and [B]o = 2.55 M. A plot of ln[A] vs. time has a slope of -10.31. What will the rate of this reaction be when [A] = [B] = 0.371 M?

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Consider the following reaction at 277 K: A + 2B â C + D where rate = k[A][B]2. An experiment was performed where [A]o = 0.00205 M and [B]o = 2.55 M. A plot of ln[A] vs. time has a slope of -10.31. What will the rate of this reaction be when [A] = [B] = 0.371 M?

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

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Chemistry: Structure and Properties

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Consider the following reaction at 277 K: A + 2B â C + D where rate = k[A][B]2. An experiment was performed where [A]o = 0.00205 M and [B]o = 2.55 M. A plot of ln[A] vs. time has a slope of -10.31. What will the rate of this reaction be when [A] = [B] = 0.371 M?