Experiment [NO] (M) C2l (M)Initial rate of increase in NOCI] (M/s) 0.0035 0.0105 0.0105 0.0100 0.0200 0.0100 9.0 x 10-6 1.6 x 104 0 x 10

The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic gas CO(g) + Cl2(g) → COCl2(g) From the following data, obtained at 360 K, determine: a) The order of the reaction, and the reaction rate law b) The value of the reaction rate constant, k c) The initial reaction rate for the formation of COCl2 when the concentration of CO is 0.30 M and that of Cl2 is 0.40 M The following data were obtained for the reaction of carbon monoxide with chlorine, producing phosgene, COCl2, a highly toxic…

The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl]. At 550°C, k = 3.2 x 10-2 sec-1. What is the half-life for this reaction? What was the initial concentration of ethyl chloride if after one minute, 0.01 M remains?

In a study to determine the rate of the following reaction: 2NO (g) + 0, (g) → 2NO, (g) the concentration of NO was 0.0450 Mat t = 5.0 s and 0.0225 Mat t= 650.0 s. What is the average rate of the reaction during this time period?

The reaction described by H, (g) + L,(g) 2 HI(g) has an experimentally determined rate law of rate = k [H2] [I2] Some proposed mechanisms for this reaction are: Mechanism A k1 (1) H,(g) + L,(g) → 2 HI(g) (one-step reaction) Mechanism B k1 =2 I(g) k_1 (1) L(g) ; (fast, equilibrium) k2 (2) H, (g) + 2 I(g) 2 HI(g) (slow) Mechanism C k1 = 2 I(g) (fast, equilibrium) (1) k2 (2) I(g) + H, (g) HI(g) + H(g) (slow) (3) H(g) + I(g) → HI(g) (fast) Question Sourc

A2 -> 2A (slow) 2A + B2 -> 2AB (fast) What is the rate law for the overall reaction?

13.102 Chlorine oxide (CIO), which plays an important role in the depletion of ozone (see Problem 13.101), decays rapidly at room temperature according to the equation 2C10(g) Cl₂(g) + O₂(g) From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) 0.12 x 10-³ 0.96 x 10-³ 2.24 x 10-³ 3.20 x 10-³ 4.00 x 10-³ [CIO] (M) 8.49 x 10-6 7.10 x 10-6 5.79 x 10-6 5.20 x 10-6 4.77 x 10-6

Consider the hypothetical reaction A(g)  +  B(g)                  C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. Which of the containers, W,X,Y or Z, would have the greatest reaction rate? Justify your answer.

Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction 2NO (g) → N₂O₂ (g) step 1 2 N₂O₂(g) + O₂ (g) Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. 2NO₂ (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. << Note: your answer should not contain the concentrations of any intermediates. rate constant 0 k₁ k₂ rate = k 1-0 010 X S