The table contins concentration data and the initial rate data for the reaction 2NO(g) + H₂(g) → N₂() + H₂O(g) Determine the rate law of the reaction. *

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0092 M-s : 2 HI (g) - H, (g) +L, (g) Suppose a 450. mL flask is charged under these conditions with 150. mmol of hydrogen iodide. After how much time is there only 75.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. dlo x10 8. 미

for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction

Given the following data, determine the rate constant of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) Experiment [NO] (M) |Ck] (M) Rate (M/s) 0.0300 0.0100 3.4 x 104 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 104

Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,Cl, (g) · SO2(g) + Cl, (g)

The mechanism for the reaction described by NO₂(g) + CO(g) → CO₂(g) + NO(g) is suggested to be k₁ (1) 2 NO₂(g) NO₂(g) + NO(g) k₂ (2) NO3(g) + CO(g) → NO₂(g) + CO₂(g) Assuming that [NO] is governed by steady-state conditions, derive the rate law for the production of CO₂ (g). rate of CO₂ (g) production =

The following reaction was studied at 25°C. The following results were obtained. a) What is the rate law for this reaction at this temperature? b) What is the value of the rate constant? Be sure to include the correct units in your answer.

Chlorine monoxide accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, ClO decomposes according to the equation:  picture The second-order rate constant for the decomposition of ClO is 6.78×109 M–1s–1 at a particular temperature. Determine the half-life of ClO when its initial concentration is 1.46×10-8 M .