Determine the value of k_c for the following reaction if the equilibrium concent

Question

Determine the value of k_c for the following reaction if the equilibrium concentration are as follows: [P_4 O_10]_eq = 2.000 moles, [P_4]_eq = 3.000 moles, [O_2]_eq = 4.000 M. P_4 O_10 (s) = P_4(s) + 5 O_2 (g) 1.320 1024 4.000 20.00 1536 In a reaction mixture confining only reactants. what is the value of Q? It cannot be determined without concentrations The following reaction is exothermic. Which change will shift the equilibrium to the left? 2 SO_2 (g) + O_2(g) -2 SO_3 (g) removing O_2 raising the temperature adding SO_3 all of the above none of the above Which of the following statements is TRUE? If Q > K. it means the forward reaction will proceed to form more products If Q

Explanation / Answer

(10)

P4O10 (s) -----------> P4 (s) + 5 O2 (g)

Equilibrium constant expression can be written as,

Kc = [P4][O2]5/[P4O10]

But, [solids] = [liquids] = 1

so, [P4O10] = [P4] = 1

So, Kc = [O2]5

Kc = (4.000)5

Kc = 1024.

So, the answer is (b)

(11) Since there are no products, Q = 0, Because, Q = [Products]/[Reactants]

So, the answer is (d)

(12)

(d) All the above

Removing of reactants (O2) , Addition of Products (SO3) shifts the equilibrium towards left side.

SInce the forward reaction is exothermic, increase in temperature shifts the equilibrium towards endothermic side i.e left side.

(13)

(c) If Q = K, the reaction is said to be at equilibrium.

(14)

(b) When a system at equilibirum is disturbed, the system shifts in a direction that minimizes the disturbance.

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