Consider the following reaction and initial rate data: 2H2 (g) + 2NO (g) → 2H,0 (g) + N, (g) [NO]initial (M) Experiment [H]nitiat (M) Initial Rate (M/s) 1 0.212 0.136 0.0248 0.212 0.272 0.0991 3 0.424 0.544 0.793 4. 0.848 0.544 1.58

For the chemical reaction NO2(g) + CO(g) → NO(g) + CO2(g) The following initial rate data were obtained Initial [NO₂] Initial [CO] Initial Rate Experiment (mol/L) (mol/L) (mol/L.s) 1 0.10 0.10 0.0050 2 0.40 0.10 0.080 3 0.10 0.20 0.0050 What is the rate law for the reaction? R = k [NO₂]4[CO] R = k [NO₂][CO] R = k [NO₂]²[CO] none of the answers are correct OR = K [NO₂]²

Given the following reaction and experimental data:   2NO(g) + Br2(g) -->  2NOBr(g)        Find the rate law. Exp [NO] (M) [Br2] (M) rate (M/s) 1 0.1 0.1 12 2 0.1 0.2 24 3 0.2 0.1 48 4 0.3 0.10 108   Group of answer choices rate = k[Br2][NO] rate = k[Br]^2 [NO]^2 rate = k[Br][NO]^2 rate = k[Br]^2[NO]

The data below were collected for this reaction: CH3Cl (g)         +     3 Cl2(g)     →        CCl4 (g)              +              3 HCl (g)   Expt. [CH3Cl] (M) [Cl2] (M) Initial Rate (M/s) 1 0.050 0.050 0.014 2 0.100 0.050 0.029 3 0.100 0.100 0.057   Provide the rate law for this reaction. Include the numerical value of the specific rate constant, k.     Rate = - Δ [Cl2]3 / Δ t     Rate = Δ [HCl] / 3 Δ t     Rate = k [CH3Cl] [Cl2]2     Rate = -Δ [CH3Cl] / 3 Δ t     Rate = 5.7 [CH3Cl] [Cl2]

A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H, initial rate of reaction х10 1.26 M 0.560 M 76.0 M/s | M/s 1.26 M 0.272 M | M/s 5.70 M 0.124 M

The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[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 = From these data, the rate constant is M-1s-1.

Using the data in the table, determine the rate constant of the reaction and select the appropriate units. k= A + 2BC+D 1.6 Incorrect Trial [A] (M) [B] (M) Rate (M/s) 1 0.350 0.320 2 0.350 0.640 3 0.700 0.320 Units Incorrect 0.0102 0.0102 0.0408 M-2S-1

The decomposition of nitrosyl bromide is followed                         2 NOBr → 2 NO + Br2   Time (s) [NOBr] (M) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033    Determine the average rate over the entire experiment.

50. The tabulated data were collected for this reaction: 19mmlich CH3 Cl(g) + 3 Cl₂(g) → CCl4 (g) + 3 HCl(g) [CH3CI] (M) 0.050 0.100 0.100 0.200 [Cl₂] (M) 0.050 0.050 0.100 0.200 ME Initial Rate (M/s) 0.014 0.029 0.041 0.115 Write an expression for the reaction rate law and calculate the value of the rate constant, k. What is the overall order of the reaction?

Consider the reaction A + 2B = C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [A] [B] (M) (M) 0.20 0.010 4.8x10-4 2 0.20 0.020 9.6x10-4 3 0.40 0.010 1.9x10-3 Trial 1 Rate (M/s) What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B].