(a)
Interpretation : The intermediate needs to interpret the given mechanism of the decomposition of hydrogen peroxide.
Concept Introduction :
The area of chemistry that deals with the rate of the
(b)
Interpretation : The rate-determining step of the given mechanism should be determined if the rate law of the decomposition of hydrogen peroxide is given as:
Concept Introduction :
The area of chemistry that deals with the rate of the chemical reaction is known as chemical kinetics. The active masses of the reactants involved in the chemical reaction are expressed by the rate law. The rate constant is a constant of proportionality between the rate and the reactant's active mass. The total of the basic stages in the chemical equations can be the overall reactant.
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CHEMISTRY: THE MOLECULAR NATURE OF MATTE
- The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?arrow_forwardThe label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?arrow_forwardDefine stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.arrow_forward
- 6a onlyarrow_forward(a) Consider the following (overall) chemical reaction k A B The experimentally determined rate law expression reads: rate = k[A]. At 30 °C, the value of k is 3 x 10-4 s¹. Let the initial concentration of A be [A]0 = 0.75 mol L-¹. The reaction should proceed until only 2% of the initial amount of A is present in the reaction mixture. (i) How long will this take at 30°C? (ii) What value would the rate coefficient k have to be, in order for the concentration of A to reach the 2% level in 1 hour? (iii) At what temperature will k reach the value you calculated in (ii) assuming that the activation energy is 40 kJ mol¹?arrow_forward(a) For a reaction, A + B > Product, the rate law is given by,Rate = k [A]1 [B]2 . What is the order of reaction?(b) Write the unit of rate constat ‘k’ for the first order reaction.arrow_forward
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- Acetone is one of the most important solvents in organicchemistry, used to dissolve everything from fats and waxes toairplane glue and nail polish. At high temperatures, it decom-poses in a first-order process to methane and ketene(CH2=C=O). At 600C, the rate constant is 8.7x10^-3s⁻¹.(a) What is the half-life of the reaction?(b) How long does it take for 40.% of a sample of acetone todecompose?(c) How long does it take for 90.% of a sample of acetone todecompose?arrow_forwardFor the reaction: 2N2O5(g) -->4NO(g) + O2(g) (a) write the mathematical rate expression in terms of (i) the disappearance of N2O5 (Reactant); (ii) the formation of NO (Product); (iii) the formation of O2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.) For the reaction: 5 Br-(aq) + BrO3-(aq) + 6 H+(aq)--> 3 Br2(aq) + 3 H2O(l); (a) write the expressions of the reaction rates mathematically in terms of (i) the disappearance of Br- (Reactant); (ii) the disappearance of BrO3- (Reactant), and (iii) the formation of Br2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A…arrow_forward5*) a) The reaction A B has been experimentally determined to be second order. The initial rate is 0.0100 M/s at an initial concentration of [A] of 0.100 M. What is the initial rate at [A]o = 0.500 M? b) The reaction below was experimentally determined to be first order with respect to O2 and second order with respect to NO. O2(g) + 2 NO(g) → 2 NO2(g) The diagrams provided represent reaction mixtures in which the number of each type of molecule represents its relative initial concentration. Which mixture has the fastest initial rate? Explain. KEY: = 02 = NO (i) (ii) (iii)arrow_forward
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