The correct option is first.
Explanation : Br- act as a catalyst which increases the rate rather than decrease it.
The decomposition of hydrogen peroxide (H2O2(aq)) is proposed to follow a reaction mechanism of Step 1:...
help me pleaseee Question 24 (1 point) A substance (A) reacts to form another substance (B): 3 A(g) = 2 B(8) The reaction is run at a particular temperature with the concentrations of A and B monitored over time and plotted in the graph. At what time was equilibrium first reached and what is the approximate value of the equilibrium constant? 2.0 16 IR [B] concentration/M 10 08 0.6 0.4 0.2 0.0 0 [A] 10 20 60 70 80 90...
1. The mechanism for hydrogen peroxide decomposition is thought to occur in two step: step 1: H2O2+ I ------> IO + H2O step 2: IO + H2O2 --------> I + H2O + O2 a. describe each step in the mechanism as unimolecular ,bimolecular or termolecular ? b. which species in the mechanism acts as an intermediate.? c. which species in the mechanism acts as catalyst.? d. what is the net reaction?
The following mechanism, proposed for the decomposition of hydrogen peroxide is composed of 2 elementary steps: H2O2(aq) + I'(aq) > H2O(l) + 10 (aq) 10 (aq) + H2O2(aq) -> H2O(l) + O2(g) + I'(aq) The rate law predicted by the mechanism is slow fast a) rate = k [H2O2) b) rate =k [H202][I] c) rate =k [H2O2][10] d) rate = k [H202) [1]
13.108. 13.109. 13.102. A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: H2O2(g) + 2 OH(g) H2O2(g) + OH(g) → H2O(g) + HO2(g) HO2(g) + OH(g) → H2O(g) + O2(g) පිපිළි 13.110. If the rate law for the reaction is first order in H2O2, which step in the mechanism is the rate-determining step?
please help as soon as possible ergent Question 24 (1 point) A substance (A) reacts to form another substance (B): 3 A(9) 2 B(9) The reaction is run at a particular temperature with the concentrations of A and B monitored over time and plotted in the graph. At what time was equilibrium first reached and what is the approximate value of the equilibrium constant? 2.0 16 [B] LO concentration/M 10 IA] 04 00 • 30 20 x 50 60 90...
A mechanism for the catalyzed decomposition of H2O2 is given below: step 1: H2O2(aq) + I−(aq) ➝ H2O(ℓ) + IO−(aq) step 2: IO−(aq) + H2O2(aq) ➝ H2O(ℓ) + O2(g) + I−(aq) Which species is the intermediate?
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq) ------> H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3min-1. If the initial concentration of H2O2 is 5.52×10-2 M, the concentration of H2O2 will be 1.56×10-2 M after _____ min have passed.
The reaction mechanism that has been proposed for the decomposition of H2O2 by iodide ion is: H2O2 + I- → H2O + IO- (slow) H2O2 + IO- → H2O + O2 + I- (fast) Which one of the following statements is true? Select one: a. The reaction is second order with respect to I-. b. I- is an intermediate. c. The reaction is first order with respect to I-. d. IO- is a catalyst. e. The reaction is zero order...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3 min-1. If the initial concentration of H2O2 is 5.66×10-2 M, the concentration of H2O2 will be 9.34×10-3 M after _______ min have passed.
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...