•Using the data from Table 2, you can now solve for the rate law exponents (m, n, p).
•To do this, you will compare the data from two experiments, where the concentration of one reactant changes and all others are held constant. (Like we did in lecture)
•Your exponents should be a whole number (0,1,2,3)
Rate = k [C3H6O]m [I2]n [H+]p
Found:
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•Using the data from Table 2, you can now solve for the rate law exponents (m,...
•Using the data from Table 4: Reaction Rate Constants, you can now calculate the activation energy for the reaction. •Calculate the activation energy using the equation below. •You will calculate the activation energy 3 times by using the data from: •Reactions 1+5 •Reactions 1+6 •Reactions 5 + 6 •You will calculate the average activation energy for the reaction. k1 Ea 1 1 In ( ) T Where: ki = rate constant at T1 kzi = rate constant at T2 T1...
Please help me solve page 2 and 3 Data Table 1 Mixture 4 Mixture1 Mixture 2 Mixture 3 Volume of 4.00M Acetone (C3H6O) Volume of 1.0OM HCI Volume of 0.00500M I Volume of H20 10.0ml 20.0mL 10.0mL 10.0mL 10.0mL 20.0mL 10.0mL 10.0mL 5.0mL 10.0ml 10.0mL 10.0mL 10.0mL 25.0mL 10.0mL 20.0mL 50.0mL 50.0mL Total Volume (mL) 50.0mL 50.0mL ec 2.07m4.2 sec 2-24 mi21344s 24-8 5%0 4-51 mine 270-66e 241 218K-24-852 Reaction Time (s) 24-65C 24 850C Mixture Temperature (°C) Concentration and...
please use the tables to solve the questions 2. Write the rate law for the reaction based on the Part 1 experimentally determined exponents rounded to the nearest integer. Specify the order of the reaction for each of the components and the overall order. 3. Calculate the rate constant, k, with appropriate units for each reaction mixture using the experimental rate law. All work must be shown for Mixture 1 in order to receive complete credit. Complete Table Ri, below....
2. Consider the second order reaction 2NOB → 2NO+ Br2 The rate constant is 0.80 M-1 5-1. The initial concentration is 0.86 M. 4) Find the half-life of the reaction. 5) Find the concentration of PH3 after 10 min. 6) How long will it take for the concentration of PH3 deceased to 0.01 M. how transcribed image text
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate constant. a. The rate constant of a first-order reaction is 2.43 × 10–2 min–1. What is the half-life of the reaction? (2 points) b. A first-order reaction has a rate constant of 0.547 min-1. How long will it take a reactant concentration 0.14 M to decrease to 0.07 M? (2 points) c. The half-life of a first-order reaction is 5.47 min. What is the...
8. Using the data provided in the table, a) write the rate law and b) determine the value of the rate constant k for the following reaction: CO(g)+ CI2(g)COC12(g) [COl, (M) C2l, (M) Initial Rate (M/s) 0.25 0.50 0.25 0.40 0.80 0.80 0.696 3.94 1.97
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 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between A and B, aA+bB⇌cC+dD The dependence of the...
Question 3 (Mandatory) (5 points) The rate constant of a first-order decomposition reaction is 0.0147 s. If the initial concentration of reactant is 0.178 M, what is the concentration of reactant after 30.0 seconds? a) 8.72 x 10 M Ob) 0.0785 M Oc) 0,115 M O d) 0.643 M e) 0.0645 M Question 4 (Mandatory) (5 points) The reaction quotient, . for a system is 1.6 x 104. If the equilibrium constant for the system at some temperature 8.5 x...
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 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between Aand B, aA+bB⇌cC+dD The dependence of the reaction...
The rate law for a general reaction involving reactant A is given by the equation rate = k[A]?, where rate is the rate of the reaction, k is the rate constant, [A] is the concentration of reactant A, and the exponent 2 is the order of reaction for reactant A. What is the rate constant, k, if the reaction rate at 450.°C is 1.23x10-1 mol/L.s when the concentration of A is 0.220 mol/L? 1/Mos When heated to 75°C, 1 mole...