The initial rates method can be used to determine the rate law for a reaction. Using the data for the reaction shown below, what is the rate law expression for the reaction? mo A+B C Trial [A](ml) [B](mol) A[A] mol (mol) At L s 1 0.065 0.065 2.29311875 × 10-7 2 0.065 0.078 2.29311875 × 10-7 3 0.078 0.065 3.9625092 × 10-7 • Write the rate law expression using two significant figures for the rate constant, do NOT include units. • Use brackets for any needed concentrations ([A], [B], or [C]). • Simplify the expression as much as possible. Do NOT use exponents of 1 or 0. Provide your answer below: rate =

The initial rates method can be used to determine the rate law for a reaction. Using the data for the reaction shown below, what is the rate law expression for the reaction? mo A+B C Trial [A](ml) [B](mol) A[A] mol (mol) At L s 1 0.065 0.065 2.29311875 × 10-7 2 0.065 0.078 2.29311875 × 10-7 3 0.078 0.065 3.9625092 × 10-7 • Write the rate law expression using two significant figures for the rate constant, do NOT include units. • Use brackets for any needed concentrations ([A], [B], or [C]). • Simplify the expression as much as possible. Do NOT use exponents of 1 or 0. Provide your answer below: rate =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096
Write rate law for the chemical reaction ?
Q4
6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
What are products of the following reaction
Use this data to determine the value of the rate constant. Ex # [A] (M) [B] (M) Rate (M/hr) 1 .240 .120 2.00 2 .120 .120 .500 3 .240 .0600 1.00 Question 4 options: 289 per hour 579 per hour 8.3 per hour 0.0144 per hour 69.4 per hour .00346 per hour 0.060 per hour 0.0173 per hour 17 per hour 0.12 per hour
How would you find the rate law for this question?
[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.