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Find the rate law and rate constant for the following reaction. A+2B-> 3C + D. rate [A] [B] (M/s) (M) (M) 1.4 x 10–2 1.00 1.00 7.5 x 10–3 1.00 0.50 6.1 x 10–2 2.00 1.00
8. The rate law for the reaction H2O2 + 2H+212 + 2H2O is rate-k[H202][1]. The following mechanism has been suggested. H2O2+1 - HOI + OH - slow OH + H H20 fast HỘI + H+ + + I2 + H2O fast Identify all intermediates included in this mechanism. A) H and I D) Honly B) H and HOI E) H20 and OH C) HOI and OH 9. Which of the following statements is false? A) A catalyst increases the rate...
10. Consider the reaction A + 2B → C ne rate law for this reaction is on der in and and order in B if the rate constant at 25°C is 1.25x 105 , find the rate of reaction when the concentration of A is 0.27M and the concentration of B is 0.32 M UMA 21 11. Consider the reaction A +2B C + D. The rate law for this reaction is first order in A and zeroth order in...
The second-order reaction, 2 Mn(CO)_5 rightarrow Mn_2 (CO)_10 is found to have a rate constant equal to 512 M^-1 S^-1. If the initial concentration of Mn(CO)_5 is 0.011 M, how long will it take for the reactant concentration to reach 0.0011 M? Units: s a. 1.6 b. 5.1 c. 0.020 d. 0.28 A plot of a 1/[A] versus time gave a straight line. This indicates that A rightarrow B + C a. the reaction is zero order in reagent A...
Which statement below is true only for a homogeneous catalysts? a. A homogeneous catalyst increase the rate of reaction by providing an alternative pathway with a lower activation energy. b. A homogeneous catalyst is a solid substance to which liquid or gaseous reactants will adhere to the surface of the catalyst. c. A homogeneous catalyst is when the catalyst is in the same physical state as the reactant. d. A homogeneous catalyst will eventually be consumed in a chemical reaction.
9. The reaction 3C A + 2B occurs in one step in the gas phase. In each blank below, write the exponent of the concentration in the FORWARD rate law or write none if that concentration does not appear in the rate law. [A] ........... [B] .......... [C] ...........
For the reaction A + 2B → C + D, the rate law is found to be rate = k[A][B]. The following mechanism, is proposed to explain the reaction. l+B→C+D a) Show that the proposed mechanism is consistent with the stoichiometry of the reaction. b) Which step must be the rate determining step? c) What is "T" called? Ca ta y st
Can someone help me? A catalyst can not increase the rate of a reaction W. by lowering the activation energy of the reverse reaction X. by lowering the overall activation energy (Eg) of the reaction Y. by changing the value of the frequency factor (A) Z. by providing an alternative pathway with a lower activation energy W.X only All of these are ways that a catalyst might act to increase the rate of the reaction 0 W,X,Y Zonly OX,Z
The initial reaction rate for the elementary reaction A+2B-3C was measured as a function of temperature when the concentration of A was 2.5 M and the concentration of B was 1 M; the measurements are summarized in the table below. From these data, a) What is the activation energy? b) What is the frequency factor? c What is the rate constant as a function of temperature using T300K as the base case? Table 1: Experimental data T (K) 310 330...
For the hypothetical reaction 2A + B --> 3C + D, the rate was determined to be: rate = k[A]3[B]1. What is the order of reaction with respect to A? _______ with respect to B? _______ What is the overall order of the reaction? __________