Use the References to access important values if needed for this question. Consi

Question

Use the References to access important values if needed for this question. Consider the following system at equilibrium where .198 ki, and Kc = 34.5 , at 1.15x 103 K: 2SO2 (g) + 02 (g)=_ 2 SO3 (g) If the TEMPERATURE on the equilibrium system is suddenly increased The value of K.[-] A. Increases B. Decreases C. Remains the same The value ofa(_JAls greater than Kc B. Is equal to K C. Is less than K The reaction must: A Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium C. Remain the same. Already at equilibrium. A. Increase. B. Decrease. C. Remain the same. The concentration of O2 will: Subriit Answer Retry Entire Group 9 more group attempts r Prevw re Te

Explanation / Answer

First, let us define the equilibrium constant for any species:

The equilibrium constant will relate product and reactants distribution. It is similar to a ratio

The equilibrium is given by

rReactants -> pProducts

Keq = [products]^p / [reactants]^r

For a specific case:

aA + bB = cC + dD

Keq = [C]^c * [D]^d / ([A]^a * [B]^b)

a)

reaction is exothermic, therefore, it releases heat

if T increases, K must decreases, since heat will not favour products

b)

Qc will then favour reactants, i.e. decreases

Qc < K, in order to fvour products

c)

rund backwards/reverse, to favour the counterbalance

d)

O2 must increases, since SO3 is reacting in reverse

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