The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂ F - is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n (don't enter 1) and concentrations taken to the zero power do not appear. Rate = S In an experiment to determine the rate law, the rate constant was determined to be 1.31 x 10-4 M¹s¹. Using this value for the rate constant, the rate of the reaction when [NO₂] = 4.92 M and [F2] = 4.59 M would be M/s.

3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096

The reaction of nitrogen dioxide with fluorine 2NO2+F2-->2NO2F is first order in NO2 and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n, 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 .

The rate of a certain reaction is given by the following rate law: rate =k[N,][H,° Use this information to answer the questions below. What is the reaction order in N,? x10 What is the reaction order in H2? What is overall reaction order? Continue ©2022 McGraw Hill LLC. All Rights Reserved.

Q2

Suggest a mechanism behind the reaction    NO(g) + Cl2(g)  à  NOCl(g)  + Cl(g) with the rate law    rate = k [NO]2 [Cl2]   This reaction cannot be a one step reaction because of its rate law. It is therefore a multistep reaction, where the slow step represents a reaction between 2 molecules of NO with one molecule of Cl2                 (slow)       2NO   +   Cl2    à   ……….                  (fast).                                à  …………                                NO     +     Cl2.     à    NOCl    +    Cl

The rearrangement of cyclopropane to propene at 500 °C(CH2)3CH3CH=CH2is first order in (CH2)3. During one experiment it was found that when the initial concentration of (CH2)3 was 0.170 M, the concentration of (CH2)3 dropped to 0.0491 M after 1304.0 s had passed.Based on this experiment, the rate constant for the reaction is ______s-1.

A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻  because it is first order for I - . After you find the reaction order for S2O82⁻  you need to calculate k.   S2O82⁻ (aq) + 3 I⁻ (aq)  →   2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 )  0.30 0.42 4.54  0.44 0.42 6.65     Rate = 120 M-2s-1 [S2O82⁻]2[I⁻]     Rate = 195 M-3s-1 [S2O82⁻]2[I⁻]     Rate = 86 M-2s-1 [S2O82⁻][I⁻]     Rate = 23 M-1/2s-1 [S2O82⁻][I⁻]     Rate = 36 M-1s-1 [S2O82⁻][I⁻]

The reaction of IC1 with hydrogen 2IC1 + H₂ → I2 + 2HCl is first order in IC1 and third order overall. 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 =

The gas phase reaction of hydrogen with iodine H₂ + 12 → 2 HI is first order in H₂ and first order in 12. Complete the rate law for this reaction in the box below. Use the form K[A]”[B]". If mor n are 1, don't enter the 1. Omit concentrations taken to the zero power. Rate =