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VISUALIZATION Determining the Rate Equation Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.262 0.995 0.539 Trial 2 0.524 0.995 0.539 Trial 3 0.262 1.99 1.08 Trial 4 0.242 0.513 0.278 Rate = K[A]°[B]! X L/mol min Recheck Next (5 of 5) 4th attempt Submit Answer Try Another Verslon 2 item attempts remalning

VISUALIZATION Determining the Rate Equation Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.262 0.995 0.539 Trial 2 0.524 0.995 0.539 Trial 3 0.262 1.99 1.08 Trial 4 0.242 0.513 0.278 Rate = K[A]°[B]! X L/mol min Recheck Next (5 of 5) 4th attempt Submit Answer Try Another Verslon 2 item attempts remalning

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 30E: The reaction 2I-(aq)+S2O82-(aq)I2(aq)+2SO42-(aq) was studied at 25C. The following results were...
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VISUALIZATION Determining the Rate Equation Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.262 0.995 0.539 Trial 2 0.524 0.995 0.539 Trial 3 0.262 1.99 1.08 Trial 4 0.242 0.513 0.278 Rate = K[A]°[B]! X L/mol•min Recheck Next (5 of 5) 4th attempt Submit Answer Try Another Verslon 2 item attempts remalning
Transcribed Image Text:VISUALIZATION Determining the Rate Equation Now that the order for both reactants is known, the rate constant, k, can be determined. Each of the four trials can be used to calculate k and then the four results can be averaged. We will use Trial 4 to determine the rate constant in this example. What is the value of the rate constant? [A], mol/L [B], mol/L rate, mol/(L-min) Trial 1 0.262 0.995 0.539 Trial 2 0.524 0.995 0.539 Trial 3 0.262 1.99 1.08 Trial 4 0.242 0.513 0.278 Rate = K[A]°[B]! X L/mol•min Recheck Next (5 of 5) 4th attempt Submit Answer Try Another Verslon 2 item attempts remalning
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