Kinetics Test-7

4. 3) The data given in the table below is for the following reaction (run at 25°C): 2 NO + O, → 2 NO, 2(g) 2(g) Initial Concentration (M) Initial rate Experiment Mol/(L s) NO 02 0.0010 7 X 10-6 1 0.0010 0.0010 0.0020 14 X 10-6 0.0010 0.0030 21 X 106 0.0020 0.0030 84 X 10-6 0.0030 0.0030 189 X 10-6 1. Determine the orders of the reaction with respect to NO and O, (show all work): NO O2

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…

The following reaction energy diagram depicts another key atmospheric reaction. Label the axes, Ea (fwd), Ea (rev). and AH rxn, and transition state, and calculate the Ea (rev). * 20H 3 78 kJ 6 72 kJ O+ H20 2 1 = Potential energy; 2 = Reaction progress; 3 = Ea (fwd); 4 = transition state; 5 = Ea (rev); 6 =AH rxn; Ea (rev) = 6 kJ 1 = Potential energy; 2 = Reaction progress; 3 = Ea (rev); 4 = transition state; 5 = Ea (fwd); 6 =AH rxn; Ea (rev) = -6 kJ 1 = Reaction progress; 2 =Potential energy ; 3 = Ea (fwd); 4 = transition state; 5 = Ea (rev); 6 =AH rxn; Ea (rev) = 6 kJ 1 = Reaction progress; 2 =Potential energy ; 3 = Ea (rev); 4 = transition state; 5 = Ea (fwd); 6 =AH rxn; Ea (rev) = -6 kJ

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Question 53?

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3:59 2A Consider the multistep reaction. What is the best rate law for the overall reaction? + Question 12 of 13 B k₁ B) Rate = k₂[C] ↑ k2 11 A) Rate = k₁[A] [B][C] C) Rate = = k₁[A]²[B] O 2E + Submit DL Doto – (1 CAT[D]\//L (CU) Tap here or pull up for additional resources D (slow) (fast)

tion 1 of 19 The decomposition of N, O, can be described by the equation 2 N,0, (soln) 4 NO, (soln) + O,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. t(s) [N,O;] (M) 2.194 175 1.965 506 1.596 795 1.331 Given the data, calculate the average rate of reaction for each successive time interval. Question Source: MRG - General Chemistry | Pub | privacy policy |help about us terms of use contact us careers N W prime video

Login | Student Veri... Bb Logout MyProgrammingLab O KINETICS AND EQUILIBRIUM Using a rate law The rate of a certain reaction is given by the following rate law: ate = k[N,J°[H_]° Use this information to answer the questions below. What is the reaction order in N,? x10 What is the reaction order in H,? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of M. reaction is 81.0 M/s. What would the initial rate of the reaction be if the concentration of N, were halved? Be sure S. your answer has the correct number of significant digits. The rate of the reaction is measured to be 7.0 x 10 M/ s when [N,] = 0.37 M and [H] = 0.32 M. Calculate the value of -1 k = || M the rate constant. Be sure your answer has the correct number of significant digits. Check Explanation O 2020 McGraw %24

Consider the gas-phase reaction between nitric oxide and oxygen showing the initial concentrations of the reactants at a certain temperature, T 2 NO(g) + O2(g) —> 2 NO2(g) experiment    [NO],M     [O2],M        Intial rtae of NO2 formation, Ms-1 1                       0.020       0..020                    0.057 2                        0.040      0.040                      0.455 3.                        0.040     0.020                       0.228 1. Determine the order with respect to NO, and outline reasoning. 2. Determine the order with respect to O2, and outline reasoning. 3. Calculate the rate constant and give its units at this temperature. 4. Calculate the initial rate of disappearance of O2(g) in units of M•s-1for experiment 3. 5. If this reaction follows a two-step mechanism with the first step being (a). Write an equation for the second step of the mechanism.(b). Identify the rate determining step of this mechanism and outline your reasoning.

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