[A], (M) 0.150 0.450 0.450 Using the information in the table, the value of the rate constant for the reaction 2 A(g) + B(g) →→ C(g) + D(g) is [B], (M) 0.300 0.300 0.150 Rate (M/min) 3.38 x 10 1.01 x 104 2.54 x 10. A) 0.00250 M²min¹¹ B) 7.51 x 104 M-²min¹¹ C) 2.25 x 104 min'¹ D) 0.00501 M¹²min¹¹ E) 4.56 x 10-7 M-²min¹¹

This question is a follow up to the previous question; you can use the rate law that you determined. 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] Trial [B] Rate (M) (M) (M/s) 1 0.25 0.010 7.5x10-4 2 0.25 0.020 1.5×10-3 0.50 0.010 3.0×10-3 Calculate the initial rate for the formation of C at 25 °C, if {A} = 0.393 M and {B} = 0.081 M. Enter your answer numerically and in terms of M/s.

Using the information in the table, the value of the rate constant TOP A(g) + B(g) → C(g) + D(g) is [A], (M) 0.100 0.200 0.300 [B], (M) 2.50 Jay 2.50 1.25 Rate (M/s) 0.460 0.920 1.38 A) 4.6 s¹ B) 0.046 s¹ C) 1.84 M¹s¹ D) 115 M²S-1 E) 0.42 s¹

The following data were collected for the reaction below. 2 NO (g) + O2 (g) --> 2 NO, (g) Initial Rate Experiment INO] (M) HO:1 (M) (M/s) 1. 0.0126 0.0125 1.41 X 10 2 2 0,0252 0.0125 5.64 X 102 13. 0.0252 0.0250 1.13 X 101 What is the rate when (NO] = 0.100 M and [0,] = 0.200 M? O 7.11 X 10 M251 O 2 M/s 0:0.002 M/s (0 14.2 M/s