For the reaction, 2COF_2(g) CO_2(g) + CF_4(g), K_c = 2.00 at a particular temper

Question

For the reaction, 2COF_2(g) CO_2(g) + CF_4(g), K_c = 2.00 at a particular temperature. A reaction mixture at this temperature initially contains all three gases in equal concentrations. Which is true of this reaction mixture? Q K; the reaction proceeds toward the reactants The reaction A rightarrow products obeys second order kinetics. What is the molar concentration of A remaining after 2.00 minutes if the reaction has a rate constant of 0.0482 M^- 's^-1 and the initial concentration of A is 0.379 M. 0.0655 M 0.119 M 0.366 M 8.42 M

Explanation / Answer

Q.32

Ans- Option (a)

for given reaction, all gases are present in equal concentration

[COF2] = [CO] = [CF4] = 0.33

Now Q= ( [CO] * [CF4] ) / ([COF2])2

=(0.33*0.33) / (0.33)2

= 1

and K=2

here Q<K , hence the reaction proceeds towards products.

Q.33

Answer- Option (b)

For a second order reaction, we know

[A]-1 = [A0]-1 + kt

= (0.379)-1 + (0.0482*120)

= 0.1187 M i.e. 0.119 M

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