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?
A+B→C
Trial123[A](molL)0.0650.0650.078[B](molL)0.0650.0780.065−Δ[A]Δt(molL s)2.29311875×10−72.29311875×10−73.9625092×10−7
ANSWER:
Reaction:
Data:
Trial | [A] (mol/L) | [B] (mol/L) | -Δ[A]/Δt (M/s) |
1 | 0.065 | 0.065 | 2.29311875x10-7 |
2 | 0.065 | 0.078 | 2.29311875x10-7 |
3 | 0.078 | 0.065 | 3.9625092x10-7 |
According to initial rate method, the rate law for this reaction is
where k = rate constant and x,y = reaction order of A and B
To find the reaction order of A and B, we need to compare the changes in the reaction rate (-Δ[A]/Δt) when the reactant concentrations are changed:
and
then
Then, the rate law of this reaction is
Now, we need to find the value of the constant rate (k). Using the rate law, we get
Finally, the rate law is
The initial rates method can be used to determine the rate law for a reaction. Using...
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 for the reaction? A+B→C Trial A B −Δ[A]Δt(molL s) 1 0.075 0.075 0.1350 2 0.075 0.09 0.1944 3 0.09 0.075 0.1350 Report your value of k with two significant figures.
Use the initial rates method with the given data to determine the rate law for the hypothetical reaction shown below. A+B→C Trial123[A](molL)0.0950.0950.1425[B](molL)0.0950.14250.095−Δ[A]Δt(molL s)3.846×10−88.653×10−81.298×10−7
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 for the reaction? A+BC Trial A (mol/) B(mol)/ (mol L 0.075 0.075 0.090 0.075 0.090 0.075 0.135 0.194 0.135 rate-24.0(B)2 rate-0.559 (B]2 rate-24.0[A]2 rate 0.559A12 0
need help thanks Write the rate law for the reaction: CH469) + 2 02(g) + 2 H2O(1) + CO2(g) if the order of all reactants is one. Complete the equation using brackets, I ), to represent concentration. Click in the answer box to activate the palette. rate = Write a valid equilibrium constant expression for the reaction below. Remember to use brackets, I). for concentrations, and use exponents where needed. Click in the answer box to activate the palette. H...
For the Reaction: A+B-C Use the Initial Rates Method to determine the rate law and the value for the rate constant including units Trial [A](M) [B] (M) Initial Rate (Ms) 0.100 0.150 0.250 0.100 0.300 1.000 0.200 0.150 0.500
Tutored Practice Problem 14.3.2 COUNSTOWARDS THE Use the method of initial rates to determine rate law. Close Problem A reaction is performed to study the reaction for the formation of phosgene from carbon monoxide and chlorine: CO + CI +COCI The following reaction rate data was obtained in four separate experiments. COM 10.540 1.08 [Cho MT 5.60x102 5.60X10- Initial Rate, M/s 4.05x10 30 8.10x10 30 8.10x10 30 1.62x10 29 0.540 1.08 0.111 What is the rate law for the reaction...
Method of Initial Rates Practice: You've been tasked with finding the rate constant, k, of a reaction that has the following rate law: rate = k [E]y [F] Under conditions where [F]>>[E] such that [F] is a constant, you measured the rate of the reaction at four different initial concentrations of [E] and calculated the initial reaction rate of each reaction. The data are given below. Trial [E] (× 10-6 M) [F] (M) Initial Rate (× 10-6 M/s) 1 10.0...
2. When using the method of initial rates to determine the reaction order of each individual reactant, why must data only be used in which one reactant is changing concentration but not the other reactants? 3. Briefly explain why the number of total drops being mixed in each experiment is kept constant throughout all five experiments. 4. Sketch a molecular‐level picture that illustrates why reaction rate increases when the concentration of a reactant is increased. Note – this might be...
MY S M Colligative Properties Part 1: Determination of Rate Law by Method of Initial Rates Trial 10.1 TH" HASOs. te (see) Initial Rate (M/see) 1 |5x10 2 Srio 3 m 5 M 2xD 0.0015 M 17 3 (273105 2 M 2X10 0.0015 M 52 19100 0.0661 |5x10-2 5x10-2 14005 m . 3 M sro M 0.0015 M 49 0674 4 11x10² M 2 x16 ² M4x105 m 0.0015 M 12 1077 1. Using the method of initial rates (ins...
Lab Questions 1. Use the Method of Initial Rates to determine the complete rate law for the reaction: 2 NOg)+ H2(g)-> N24g) +2 H20g) Trial [H2] 0.0100 0.0200 0.0300 0.0100 0.0100 NO Initial Rate, M/s 3.82 x 10- 7.63 x 103 1.14 x 102 1.53 x 102 3.43 x 102 20.0100 2 00100 30.0100 0.0200 0.0300 4