Consider the following mechanism for the decomposition of nitrogen dioxide NO 2(g) → NO(g) + 0(g)...
The nitrogen-monoxide-catalyzed decomposition of dinitrogen monoxide is thought to proceed by a two-step mechanism: NO(g) + N2O(g) --> N2(g) + NO2(g) (slow) 2 NO2(g) --> 2 NO(g) + O2(g) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [N2O]2 Rate = k [NO] [NO2] Rate = k [N2O]2 [N2O] Rate = k [NO2] [N2O] Rate = k [N2O] [N2O] Rate = k [NO] [N2O] (b) Choose...
The decomposition of nitrogen dioxide occurs according to the equation below: NO2 (g)------>NO( g)+1/2 O2 (g) The reaction is second order with respect to NO2. The specific rate constant for this reaction is 3.04M-1min-1. How long does it take for the concentration of NO2 to decrease from 2.00M to 1.25M?
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
The rate constant for the decomposition of nitrogen dioxide NO2(g) LaTeX: \longrightarrow ⟶ NO (g) + 1/2 O2(g) with a laser beam is 1.76 1/MLaTeX: \cdot ⋅ min. Find the time, in seconds, needed to decrease 2.4 M of NO2 to 1.18 M. Hint: What is the order of the reaction? How can you determine that? Units of k?
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
Decomposition of nitrogen dioxide into nitrogen oxide gas is an equillibrium process described by the following equation: 2NO2(g)--2NO(g)+ O2(g), deltaH=-98.7kj. Predict whether the position of equilberium will shift to the right left or no change. -increase the concentration of NO -Decrease the concentration of NO2 -Increase the pressure by the addition of helium gas -Increase the pressure by decreasing the volume - Decrease the temp -Add a catalyst
1A. The decomposition of dinitrogen monoxide (nitrous oxide) occurs in two steps. The mechanism that has been proposed is as follows: Step 1: N2O (g) à N2(g) + O(g) Step 2: N2O (g) + O(g) à N2(g) + O2(g) Write the chemical equation for the overall reaction and identify any reaction intermediates (spectators). What is the molecularity of each of the elementary (steps) reactions?
Nitrogen dioxide gas undergoes decomposition producing nitrogen monoxide and oxygen gases: 2 NO2(g)........ 2 NO(g) + O2(g) A sample consisting of 0.10 moles of NO2 is placed in a 10.0 L in a container that is then heated to 750 K. When equilibrium is reached, the pressure in the container is 0.827 bar. Calculate the equilibrium constant and the degree of dissociation at this temperature. (Hint: pressures are directly proportional to concentration, so they can be used in ICE tables).
Nitrogen dioxide and carbon monoxide react to form nitrogen monoxide and carbon dioxide, like this NO 2(g)CO (g)>NO(g)+CO2(g) Use this chemical equation to answer the questions in the table below. None Suppose 150. mmol of NO, and Some, but less than 150. mmol. 150. mmol of CO are added to an 150. mmol empty flask. How much NO will be in the flask at equilibrium? More than 150. mmol. None Suppose 155. mmol of NO and Some, but less than...
Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: rate constant elementary reaction step NO(g)+ 02(g) NO2(9) 0(g) 1 NO(g) O(g) NO2(9) k2 2 Suppose also k,»k,. That is, the first step is much faster than the second. 2* Write the balanced chemical equation for the overall chemical reaction: Write the experimentally observable rate law for the overall chemical reaction rate k Note: your answer should not contain the concentrations of any intermediates. Express the rate...