If we represent the equilibrium as: We can conclude that This reaction is: A. Ex

Question

If we represent the equilibrium as: We can conclude that This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. When the temperature is increased the equilibrium constant, K: A. increased B. Decreases C. Remains the same D More information is needed to answer this question. When the temperature is increased the equilibrium concentration of NO_2: A. increased B. Decreases C. Remains the same D More information is needed to answer this question.

Explanation / Answer

Q1

New bonds form, thereofre this requires external energy, therefore, it must be ENDOTHERMIC

HRxn = 2*No2 - N2O4 = (2*33.2) - (11.1) = 55.3

Q2

Since this is endothermic, i.e. it requires energy/temperature to go in a forward direction

then, increasing T will favour more products, so K increases

Q3.

NO2 is a product, so it must increase, as previously stated

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