**Exercise: Match the Descriptions to the Appropriate Term**In this activity, you will assign each description from the "Answer Bank" to its corresponding term: "Rate of reaction," "Rate law," or "Rate constant."### Terms:- **Rate of reaction**- **Rate law**- **Rate constant**### Answer Bank:1. **Description 1**: has different units, such as molarity per second (M/s), inverse seconds (s⁻¹), or inverse molarity-seconds (M⁻¹·s⁻¹), depending on the reaction order.2. **Description 2**: symbolized as \( k \).3. **Description 3**: a formula that relates reactant concentration to reaction rate.4. **Description 4**: always has units of amount per time (i.e., molarity per second, M/s, or molarity per minute, M/min).**Instructions**: Drag each description to the appropriate term box.This exercise will help you understand the fundamental concepts of reaction rates in chemistry.

Consider a general chemical reaction: 2A+B→3C The rate law expression for this reaction is…

Answer Bank can have different units, such as molarity per second (M/s), inverse seconds (s-¹), or inverse molarity-seconds (M-¹. s-¹); depen reaction order symbolized as k a formula that relates reactant concentration to reaction rate always has units of amount per time (i.e., molarity per second, M/s, or molarity per minute, M/min)

Answer Bank can have different units, such as molarity per second (M/s), inverse seconds (s-¹), or inverse molarity-seconds (M-¹. s-¹); depen reaction order symbolized as k a formula that relates reactant concentration to reaction rate always has units of amount per time (i.e., molarity per second, M/s, or molarity per minute, M/min)

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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please include correct units included, correct number of significant digits.
= For a different reaction X2Y, the initial [X] 1.0 M, and [Y] = 0 M. After 5 minutes the [X] has fallen to 0.8 M and then does not change any further. Draw a graph of [X] v time for the first 10 minutes. Use the blank template graph from Q1. Use the editor to format your answer
[Refe The decomposition of ozone is believed to occur in two steps: O3 02 +0 (elementary reaction) O3 +0 202 (elementary reaction) Identify any reaction intermediate. What is the overall reaction? O The O atom is a reaction intermediate. The overall reaction: 203 302 The O2 molecule is a reaction intermediate. The overall reaction: 302 203 O The O, molecule is a reaction intermediate The overall reaction; 20,- 30 The O atom is a reaction intermediate The overall reaction: 30, 202
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Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.
Consider the following kinetic data collected at the very beginning of a reaction:Run # Initial [A] Initial [B] Initial Rate of Reaction(mol/L) (mol/L) (mol/L-s)----------------------------------------------------------------1 0.10 0.10 0.00902 0.20 0.10 0.0363 0.10 0.20 0.018Which of the following is an appropriate expression for the rate law and rate constant?A0 Rate = k[A][B]; k = 0.9 L / mol-sB) Rate = k[A]2[B]; k = 0.9 L2/mol2-sC) Rate = k[A]2[B]; k = 9.0 L2/mol2-sD) Rate = k[A]4[B]2; k = 9.0 x 103 L / mol-s
tter What solid was formed: Copper (II) ions (from CuSO4) react with solid Appearance of copper sulfate: Appearance of zinc: Appearance after 10 min: Appearance after 20 min: Balanced reaction: Type of reaction: 0 min Lab 5 pg. 3 Zinc metal Cu²+ (aq) + Zn () About 10-20 mL of copper sulfate solution are added to two beakers. Note the appearance of the solution. Zinc is added to one beaker (the other is reference control). Note the appearance after 10 and 20 minutes in comparison to 0 min. (reference control). 10 min CuSO4 (aq) + 20 min Zn (s) → Ed: January 2032 ZnSO4 (aq) + Cu (s) In general, salts are soluble in water. In some cases, the forces that hold the salt together are too strong for the water molecules to pull apart. These are called insoluble salts. You can tell if you have an insoluble salt by the formation of a precipitate when combining solutions of soluble salts, or a gas is evolved (observed as gas bubbles, or a foam). For the following reactions, the indicated solutions…
Consider the reaction: 4 PH3 (g) à P4 (g) + 6 H2 (g). If, in a certain experiment over a specific time period, 0.036 mol of PH3 is consumed in a 1.0-L container each second of reaction, which of the following is correct about the production rate of H2? Choose one option only. Options: a. 0.0090 M/sec b. 0.024 M/sec c. 0.054 M/sec d. 0.216 M/sec e. None of the above
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> A Moving to another question will save this response. estion 19 Consider the reaction in aqueous solution: 3r + S20g2- → 13 + 2 SO42- Under a given set of conditions, the concentration of 13 changes from 0,0 M to 7,6 x 10-4 M in 20 seconds. Calculate A[SO2yAt (in mol/L-s) for this time interval. O -6.5 x 10-5 mol/L-s O 5.0 x 10-5 mol/L·s O 1.2 x 10-5 mol/L·s O 7.6 × 10-5 mol/L·s O -5.0 x 105 mol/L-s A Moving to another question will save this response. MacBook Air F6 F5 吕口 F4 F3 F2 F1 #3 24 % 7 6. 4. 2 00
5. The gas-phase reaction of hydrogen and iodine monochloride as shown in the following balanced equation: H2(g) + 2 ICI (g) → 2 HCI (g) + I2 (g) Initial [H2] (M) Initial [ICI] (M) Initial Reaction Rate (M/s) 1.2 x 10-6 -6 Experiment 1 0.058 0.0150 0.058 3.6 x 10 1.2 x 10-6 2 0.0450 3 0.0145 0.0150 (a) What is the reaction order with respect to each reactant? (b) What is the rate law? (d) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
please anwer with the correct sig figs and units