Determine the rate law and the value of k for the following reaction using the data provided. CO( g ) + Cl 2 ( g ) → COCl 2 ( g )
. Experiment
1, 2, 3
. Initial Rate ⁄ M · s − 1
0.696, 1.97, 3.94
. [CO] ⁄ M
0.25, 0.25, 0.50
[Cl 2 ] ⁄ M
0.40, 0.80, 0.80
Determine the rate law and the value of k for the following reaction using the data...
8. Using the data provided in the table, a) write the rate law and b) determine the value of the rate constant k for the following reaction: CO(g)+ CI2(g)COC12(g) [COl, (M) C2l, (M) Initial Rate (M/s) 0.25 0.50 0.25 0.40 0.80 0.80 0.696 3.94 1.97
CO(g) + Cl2(g) ? COCl2(g)[CO]i (M) [Cl2]i (M) Initial Rate (M-1s-1)0.25 0.40 0.6960.25 0.80 1.970.50 0.80 3.94
What concentration of CO should be used in trial 3 in order for the researcher to get enough information to determine its reaction order? CO(g)+ Cl2(g) COCI2g) Initial Rate [COli (M) Clli (M)(M-15-1) Trial 1 0.25 Trial 2 0.50 Trial 3 0.40 0.696 0.80 3.94 0.80 1.97 0.80 M 0.25 M O 0.40 M O 0.50 M
Determine the rate law and the value of k for the following reaction using the data provided. Give proper units on the rate constant. No2 (g) + O3(g) --> NO3(g) + O2 (g) [NO2]i (M) [O3]i (M) Initial Rate 0.10 0.33 1.42 0.10 0.66 2.84 0.25 0.66 7.10 Answer is Rate = 43 ^-1 S ^-1 How do you get this rate? Explain the steps. I keep getting 183.
Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + Br2(g) → 2 NOBr(g) [NO]i (M) [Br2]i (M) Initial Rate (Ms-1) 0.030 0.0055 1.81 x 10-2 0.030 0.0110 3.62 x 10-2 0.060 0.0055 7.25 x 10-2 please show step by step.
Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.033 1.84 × 10-4 0.066 7.37 × 10-4 0.099 1.66× 10-3 A. Rate = 5.6 × 10-1 M-1/2s-1[N2O5]3/2 B. Rate = 1.7 × 10-1 M-1s-1[N2O5]2 C. Rate = 1.7 × 10-1M1/2s-1[N2O5]1/2 D. Rate = 6.0 × 10-1 M-2s-1[N2O5]3 E. Rate = 5.2 × 10⁻1 s-1[N2O5]
Using the following data, determine the rate law and calculate k: rate = k[F2]x[ClO2]y Experiment [F2] (M) [ClO2] (M) Initial rate (M/s) 1 0.40 0.05 1.2 M/s 2 0.20 0.10 0.60 M/s 3 0.40 0.10 2.4 M/s
Part A Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O2(g) + 2NO2(9) [NO]; (M) [Ogl (M) Initial Rate (M4 st) 0.030 0.0055 8.55 x 103 0.030 0.0110 1.71 x 10-2 0.0055 3.42 x 10-2 0.060 Rate = 3.1 x 105 M-3 s[NO]2[0212 Rate = 57 M' s'[NO][O21 Rate = 9.4 x 103 M25 *[NO][0212 Rate = 3.8 M-1/2 s [NO](O2) 1/2 Rate = 1.7 x 103 M2 s?[NO]2[02]
Part A Determine the rate law and the value of k for the following reaction using the data provided. SO82 (aq) + 3 l'(aq) 2 SO42-() + 13 "(aq) [S,08?) (M) (0) (M) Initial Rate (M's) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 O Rate = 86 M?s" [S,08? Rate = 36 M 's' (S203 2701 Rate = 120 M2 [S208 2 101 Rate - 23 M-1/2" [S2O3 1912 Rate = 195 Mºss,Og 2012 Submit Request Answer
Part A Determine the rate law and the value of k for the following reaction using the data provided. SO82 (aq) + 3 l'(aq) 2 SO42-() + 13 "(aq) [S,08?) (M) (0) (M) Initial Rate (M's) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 O Rate = 86 M?s" [S,08? Rate = 36 M 's' (S203 2701 Rate = 120 M2 [S208 2 101 Rate - 23 M-1/2" [S2O3 1912 Rate = 195 Mºss,Og 2012 Submit Request Answer