Question

2. Consider the reaction A2+ B2 = 2AB. If the initial concentration of both A2 and B2 is 4.0 M. and after 10 minutes the reaction appears to stop. The concentration of [A2) is now 2.0M. a. Draw a graph of [A2) vs. time, over the span of 20 minutes. 09. (M concertuohon 5 15 20 time (min) b. On the same axes draw a graph of [B2] v time, over a span of 20 minutes. c. On the same axes draw a graph of [AB] v time over a span of 20 minutes. d. We can discuss the rate in terms of [A2], [B2], or (AB). How are they related to each other? - A[A2]/At = ? e. What is the difference between A[A2]/At and d[A2]/dt? Att- 15 minutes has the reaction actually stopped? Explain your answer at the macroscopic level and the molecular level.

Answer 1

Solution As per given in the question 2 The reaction is- Azt B2 Z RAB initial concentration of Az] and ($] .= 4.00 concentration of (Az] after lo minutes = 2.000 @, graph of (A2) "/s timet) including (B2] "/stand (AB] /st is — imt [46] (12),18,7 2MT (Con.) 207 1MT í lo is zo es time (in minutes) at at 167 see in above graph . re see in above graph - ® for the reaction & AB Azte Rate of Reaction= -4[42-4331 A[48] -41922. - lipcha? One minute (E) At t=10 minutes, Equilibrium is established hence after Is minute reaction will be in Equilibrium state. At Equilibrium Rate of forward Reaction becomes equal to rate of backward reaction, but the proceed in forward and backward 10 eaction, but the reaction continue and backward reaction.