The decomposition of H_2O_2 in the presence of l^- is believed So occur via the

Question

The decomposition of H_2O_2 in the presence of l^- is believed So occur via the following mechanism: Step 1: H_2O_2 (aq) + I^- (aq) right arrow H_2O (I) + IQ^- Step 2: H_2O_2 (aq) + IO^- (aq) right arrow H_2O (I) + O_2 (g) + |^- (aq) Which of the following is true of this mechanism I^- and IO^- we both intermediates I^- and IO^- are both catalysts I^- is an intermediate, and IO^- is a catalyst I^- is a catalyst, and IO^- is an intermediate Consider a single step reaction which has an activation energy of 25 kJ for the forward reaction, and an activation energy of 125 kJ for the reverse reaction. Which of the following represents All for the reaction -100kJ 100kJ 150kJ -l50kJ Which variables when plotted will yield a straight line having a slope of - E/R, (where T represent Kelvin temperature, and F is activation energy k vs 1/ T k vs T In k vs T In k vs l/T A reaction has 2 reactants A and B. As the concentration of A doubles, the rate doubles. As the concentrations of BOTH A and B are tripled, the rate increases correct by factor of 27. Which of the following is the correct order for reactant B in the rate law for the reaction third order second order first order zero order

Explanation / Answer

1) Intermediates are those which are vanished in the course of the reaction and are very difficult to extract.

Thus, the correct option is :- (d)

2) delta H = Eforward - Ebackward = 25 - 125 = -100 kJ

Thus, the correct option is :- (a)

3) The Arrhenius Equation is :- lnk = E/RT

Thus, the plot of lnk vs (1/T) will give a slope of E/R and the graph will be a straight line

Hence the correct option is :- (d)

4) rate of reaction = k*[A]n*[B]m ; where k = rate constant , n & m = order of reaction with respect to A & B respectively

Hence, the correct option is :- (a)

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