The following initial rate data are for the reaction of ICl with hydrogen: 2 ICl + H2I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1

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The following initial rate data are for the reaction of nitrogen dioxide with carbon monoxide: NO, + CO NO + CO, Experiment 1 NO:l,. M 1.28 [CO], M 0.457 0.914 Initial Rate, Ms- 1.06 1.06 lo 2 1.28 2.55 2.55 13 0.457 4.23 4 0.914 4.23 Complete the rate law for this reaction in the box below. Use the form k[A]mB]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is

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Question 13 of 26 Using the data in the table, calculate the rate constant of this reaction. A+B C + D Incorrect k= O ÏI Trial 1 2 3 Units. Incorrect [A] (M) 0.390 0.390 0.624 60°F [B] (M) 0.360 0.972 0.360 O Attempt 1 Rate (M/s) 0.0146 0.106 0.0234 10:23 PM 5/30/2022 11

Hydrogen gas reduces NO to N2 in the following reaction: 2H, (g) + 2NO(g) 2H,0(g) + N, (g) The initial reaction rates of four mixtures of H, and NO were measured at 1500°C with the following results: Experiment [H2]o (M) [NO]o (M) Initial Rate (M/s) 0.212 0.136 0.0393 2 0.212 0.272 0.0789 0.424 0.544 0.624 0.848 0.544 2.50 4.

Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O4²-(aq)→ 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 0.40 1.2 x 10-4 0.40 6.2 x 10-5 Initial rate (M/sec) 3.1 x 10-5 (a) Find the order of the reaction with respect to HgCl2₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.

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+ esc Studying the reaction A + B → Products, you gather the following information: Initial Rate (Ms¹) 0.35 0.30 0.30 3.15 0.40 0.60 22.4 What is the value of the rate constant? [A] 0.10 F1 [B] 0.30 F2 A 00 F3 3 000 000 F4 26 2 : Question 3 of 5 F5 MacBook Pro M PS F6 c « F7 A DII F8 stv D F

The following initial rate data are for the reaction of nitrogen dioxide with fluorine: 2 NO₂+ F₂2 NO₂F Experiment 1 2 3 4 [NO₂lo M 2.43 2.43 4.86 k= 4.86 Falo. M 4.25 M-¹-1 8,50 4.25 8.50 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where 1 is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate= Initial Rate, M-a 1.19 x 10 2.38 x 10-3 2.38 x 10 4.75 x 10-