he web... Google structure.com/courses/112712/assignments/144236 submit Below yo

Question

he web... Google structure.com/courses/112712/assignments/144236 submit Below you will find the kinetics data for the reaction Kc. 0.44 open up the following spreadsheet for data to be used to answer questions below: Q s KKineticsDataxlsx Question: 1. What is the value of K for this reaction? 2. For Experiment 1: 1.What are the initial conditions? 2. e the amounts of reactants increasing or decreasing? What about the products? 3. Is the reaction proceeding in the forward direction or reverse direction? 4. When does the reaction reach equilibrium and how can you tell? 3. For Experiment 2: 1. What are the initial conditions (concentrations)? 2. Are the amounts of reactants increasing or decreasing? What about the products? 3. Is the reaction proceeding in the forward or reverse direction? 4. When does the reaction reach equilibrium? How can you tell? 4, Look at the values of the IN204 fraction in the right most column for experiment NO, each 1 What do we call this fraction? 2. What is the value of K for this reaction? 3. If you were to look only at these two columns of data, how could you tell the reaction was moving toward equilibrium? 5, How is Q different from K?How arc they aliko? 6. In the spreed sheet label the column that ropresents Q and markthe point after with Q Klyou can highlight the colls and add comments to sho

Explanation / Answer

1

For this reaction,

K(equilibrium constant) or Kc( equilibrium constant expressed in terms of concentration)=

Kc=[N2O4]/[NO2]2      

   =0.44

Thus value of K for this reaction is 0.44

2

For experiment 1-

i.) The initial condition for the reaction are-

at t=0 (i e when the reaction starts)

concentration of NO2 is 1 unit

concentration of N2O4 is 0 unit

ii)The amount of reactant is decreasing(from1unit to 0.9 unit)

The amount of product is increasing (from0 unit to 0.1 unit)

iii)The reaction is proceeding in forward direction, as amount of product is increasing.

iv)Reaction reaches equilibrium at t=9th min

Because, at equilibrium the concentration of each of reactant and product becomes constant.

[after 9 min concentration of NO2 becomes 0.75 (app) units and concentration of N2O4 becomes 0.24 (app) units.]

Also, at equilibrium the rate of forward reaction(Kf) is equal to rate of backward direction (Kb) i.e.

Kf=Kb

Or,

Kf/Kb=K

And value of K=0.44 (which is constant at the given temperature . )

Note that value of K and various concentration terms are constantafter( t=9 min.)

                        

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