Question

REACTION A + B + C ---> Products Trial [A](M) [B](M) [C](M) Rate(M/s) 1 1.0 1.0...

REACTION A + B + C ---> Products

Trial [A](M) [B](M) [C](M) Rate(M/s)
1 1.0 1.0 0.010 1.0E-4
2 1.0 2.0 0.010 4.0E-4
3 1.0 1.0 0.020 2.0E-4
4 2.0 1.0 0.010 2.0E-4

Using the data in the table and the rate law below, identify the reaction order with respect to each reactant.

Rate = k[A]m[B]n[C]p

(I need to find m=?, n=?, and p=?)
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

let the rate be r= K[A] a[ B]b [C]c , where a , b, and c are orders of reaction with respect to A, B and C. K is rate constant

from 1st data point, 1*10-4= K[1]a [1]b [ 0.01]c (1)

from 2nd data point , 4*10-4 =K[1]a[2]b[0.01]c (2) Eq.2/Eq.1 gvies 4= 2b, b= 2

from 3rd data point, 2*10-4= K[1]a [1]b[ 0.02]c (3), Eq.3/Eq.1 gives 2c= 2, c=1

from 4th data point, 2*10-4 = K[2]a [1]b[0.01]c (4), Eq.4/Eq.1 , 2a=2, a=1

from Eq.1, 1*10-4= K[ 1]1[1]2 [0.01]1, K= 0.01

the rate equation becomes r= 0.01[A] [B]2 [C]

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Rate Law: Iodination of Acetone Experiment X trial   initial [A] initial [B] Rate (M/s) #1    1.00...
Rate Law: Iodination of Acetone Experiment X trial   initial [A] initial [B] Rate (M/s) #1    1.00 x 10-3 0.25 x 10-3 0.26 x 10-9 #2   1.00 x 10-3 0.50 x 10-3 0.52 x 10-9 #3   1.00 x 10-3 1.00 x 10-3 1.04 x 10-9 #4    2.00 x 10-3 1.00 x 10-3 4.16 x 10-9 #5    3.00 x 10-3 1.00 x 10-3 9.36 x 10-9 #6    4.00 x 10-3 1.00 x 10-3 16.64 x 10-9 Determine the rate law and calculate...
Trial [A] [B] Rate (M/s) 1 0.25 0.25 4.0 x 101 2 0.50 0.50 3.2 x...
Trial [A] [B] Rate (M/s) 1 0.25 0.25 4.0 x 101 2 0.50 0.50 3.2 x 102 3 0.25 1.0 6.4 x 102 4 0.50 0.75 7.2 x 102 a. Find the rate law for the reaction. b. What is the rate constant (k) with correct units? c. What would the reaction rate be when the initial concentrations of A and B are 0.75?
For the reaction A+B+C --> D Trials A B C Initial Rate (M/s) 1 0.10 0.10...
For the reaction A+B+C --> D Trials A B C Initial Rate (M/s) 1 0.10 0.10 0.10 3.0X10^-5 2 .10 .10 .30 9.0x10^-5 3 .20 .10 .10 1.2x10^-4 4 .20 .20 .10 1.2x10^-4 1. What is the reaction order with respec to A? 2. What is the reaction order with respect to B? 3. What is the reaction order with respect to C?
Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of...
Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A] (M) [B] (M) Rate (M/s) 1 0.15 0.010 2.7×10−4 2 0.15 0.020 5.4×10−4 3 0.30 0.010 1.1×10−3 Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units.
A certain second-order reaction (B→products) has a rate constant of 1.60×10−3 M−1⋅s−1 at 27 ∘C and...
A certain second-order reaction (B→products) has a rate constant of 1.60×10−3 M−1⋅s−1 at 27 ∘C and an initial half-life of 296 s . What is the concentration of the reactant B after one half-life?
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If...
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If the initial concentration of A is 0.00680 M. what is the concentration after 315 s? b.)The rate constant for this zero-order reaction is 0.0190 M·s–1 at 300 °C. A--> products. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.240 M? c.)The rate constant for this second-order reaction is 0.520 M–1·s–1 at 300 °C. A-->...
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If...
a.) The rate constant for the reaction is 0.460 M–1·s–1 at 200 °C. A--> products. If the initial concentration of A is 0.00680 M. what is the concentration after 315 s? b.)The rate constant for this zero-order reaction is 0.0190 M·s–1 at 300 °C. A--> products. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.240 M? c.)The rate constant for this second-order reaction is 0.520 M–1·s–1 at 300 °C. A-->...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
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 Part A What is the reaction order with respect to A? Part B What is the reaction order with respect to B? Part C What is the reaction order...
Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of...
Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table: Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units. Trial [A] (M) [B] (M) Rate (M/s) 1 0.35 0.010 1.5×10−3 2 0.35 0.020 2.9×10−3 3 0.70 0.010 5.9×10−3
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of...
1)A second order reaction has a rate constant of 3.7 M-1min-1. if the initial concentration of the reactant is 0.0100M, what is the concentration remaining after 15 min? a) .0099M b) .0056M c) .0025M d) .0064M 2) the rate constant for the first order decomposition of A at 500 degrees Celsius is 9.2 x 10 to the negative 3rd powers s-1. How long will it take for 90.8 % of a 0.500M sample of A to decompose a) 2.5 x...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT