Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is Rate [A]. (M) [B], (M) (M/s) A) 0.106 M-'s-1 B) 6.80 M-'s-1 1.25 0.100 0.850 0.362 s-1 1.25 0.300 2.55 D) 68 M-³ s-1 E) 1.36 s-1 3.75 0.200 5.10

Determine the rate constant for the reaction 2 A + B - C [A] (M) [B] (M) Initial Rate (M/s) 0.05 0.05 0.035 0.10 0.05 0.070 0.20 0.10 0.56 O 2.8 x 102 M-2s-1 O 14 M-2s-1 O 1.4 x 102 M-2s-1 O 1.4 x 103 M-2s1

The reaction 4 HBr(g) + O2(g)  2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results:   Experiment [HBr(g)] (M) [O2(g)] (M) Rate (M/s)   1 0.00542 0.00542 0.341 2 0.00542 0.0108 0.679 3 0.0108 0.00542 0.679 4 0.0108 0.0108 1.35 (a) What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)] Rate = k [HBr(g)]2 [O2(g)]     Rate = k [HBr(g)] [O2(g)]2 Rate = k [HBr(g)]2 [O2(g)]2 Rate = k [HBr(g)] [O2(g)]3 Rate = k [HBr(g)]4 [O2(g)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of HBr(g) is 0.00861 M and that of O2(g) is 0.0123 M if the temperature is the same as that used to obtain the data shown above? _________M/s

A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂(g) +50₂ (g) She fills a reaction vessel with Cl₂O5 and measures its concentration as the reaction proceeds: time (minutes) 0 10. [CI,Os] 0.300M 0.161M 20. 0.0864M 30. 0.0464M 40. 0.0249M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = x10 0.0 X 5

The synthesis of ammonia obeys the following reaction: N2(g) + 3H2(g) → 2 NH3(g) N2(g) concentration measurements were taken at different times and plotted. 1) What is the average reaction rate of NH3(g) between 0 and 3 hours? (Attention, the graph is in "hour" and we want a speed in "mole/L s") 2) What is the instantaneous rate of reaction of NH3(g) at the 1st hour? 3) What is the general speed between 0 and 3 hours?

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]

Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is

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]

The reaction H2 (g) + 2 NO (g) + H,O (g) is studied at a certain temperature by determining the rate of reaction at reactant concentrations. The results are as follows: N,0 (g) 2. Concentration (M) Rate [NO] (i) (ii) [H] (M/s) 0.25 0.10 0.126 0.50 0.10 0.504 (iii) 0.50 0.20 1.03 The rate law is written as Rate = k [NO]* [H]°. The exponents x and y represent the order with respect to NO and H2, respectively. Calculate the value of x and y from the data provided.