Direction: Determine whether the following statements conform to the rate law by writing True or False. _1. Rate law states that overall order of reaction can be determined by adding the reaction orders of the reactants. _2. Second order of reaction is the fastest. _3. All reactions proceed at the same rate. _4. The balance equation can be used to determine the rate of reaction. 5. The slow reactive or unreactive species in a reaction can be identified using rate law.

Direction: Determine whether the following statements conform to the rate law by writing True or False. _1. Rate law states that overall order of reaction can be determined by adding the reaction orders of the reactants. _2. Second order of reaction is the fastest. _3. All reactions proceed at the same rate. _4. The balance equation can be used to determine the rate of reaction. 5. The slow reactive or unreactive species in a reaction can be identified using rate law.

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...

See similar textbooks

Similar questions

b. On the same diagram, draw a dashed line to indicate the changes that result from the addition of the catalyst. Explain the role of the catalyst in changing the rate of the reaction. 11. Given the following initial rate data: каза гази Rate (mole/Los) 1,350 12 TI T2 13,500 T3 54,000 a. What is the rate expression for the reaction? b. What is the value for k and its units? [A] .20 .50 .50 [B] .30 .60 1.2 c. What would happen to the rate if both the concentrations of A and B were doubled? 12. Consider a reaction of the form 2A + BC. The data for this reaction is given below: Initial rate of formation of C M/s Initial [A] Initial [B]
What would happen to the rate of a reaction with rate law rate = k[NO]<[H,] if the concentration of H, were halved? O A. The rate would not change. O B. The rate would be doubled. O C. The rate would be four times larger. O D. The rate would also be halved.
A student follows the Determining the Rate Law for the Crystal Violet-Hydroxide lon Reaction procedure. The stock concentration of sodium hydroxide used in trial 1 is 0.021 M. The stock concentration of sodium hydroxide used in trial 2 is 0.010 M. Given the data below, what is the hydroxide ion concentration (M) in the trial 1 reaction mixture? Give your answer to four decimal places. Volume NaOH Volume Crystal Violet (mL) (mL) Trial 1 5.00 5.00 Trial 2 5.00 5.00
Comment how the temperature affects the rate. a. Temperature definitely has an affect on the rate. When there is an increase in temperature, the rate at which the reaction occurs also increases. This is proved through my data. As each experiment had an increasing temperature, here are my rates that go from lowest to highest temperature: 3.25*10 M/s, 4.15*10 M/s, 6.85*10 M/s, 9.17*10* M/s. With this increase in temperature, there is therefore an increase in the energy of molecules in the solution. With this increase in energy, there is an increase in collisions with enough energy, and this ultimately leads to the rate increasing.
Rate Expressions: Write the rate expression and the rates of all other species using the given rate for the stated reactions. Make sure the reactions are balanced. 3. N₂ + O₂ → N₂0s N₂ + S0₂ → N₂ 205 Rate of depletion of O₂ = 0.79M/s 4. C₂H6+ O₂-3H₂O +2CO₂ Rate of formation of CO₂= 1.32M/s 5. H₂O2)→ H₂O(g) + O2(g) Rate of formation of H₂O = 1.21M/s
Answer questions 6,7 and 8 please Answer ASAP PLEASE
Can you please find the rate law for this one in the picture?
Given the reaction and its rate law below, what happens to the rate of reaction when the concentration of NO is doubled? NO (g) + O3 (g) → NO2 (g) + O2 (g) Rate = k[NO][O3] A. The rate triples. B. The rate doubles. C. The rate halves. D. The rate quadruples. E. The rate stays the same.
The rate of a certain reaction is given by the following rate law: rate =k| N,| H2 -k[N;][H+]° Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.620 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 24.0 M / s when [N2] = 1.5 M and [H2] = 0.16 M. Calculate the value of the k = |M -2 -1 •S rate constant. Round your answer to 2 significant digits.