Consider the following equilibrium: 2O_3(g) 3O_3(g) k_eq = 65 Initially 0.10 mol

Question

Consider the following equilibrium: 2O_3(g) 3O_3(g) k_eq = 65 Initially 0.10 mole of O_3 and 0.10 mole of O_2 are placed in 1.0 L container Which of the following described the change in concentrations as the reaction proceeds toward equilibrium? Which of the following applies lo a chemical equilibrium? Forward and reverse reaction rates are equal Equilibrium can be achieved from either direction Macroscopic properties are constant I only I and II only II and III only I. II and III In which of the following will the driving forces of minimum enthalpy and maximum entropy oppose one another? 2C(s) + O_2(s) rightarrow 2CO(g) delta H = -221kJ 2N_2(g) + O_2(g) rightarrow2N_2(0) delta H = +164 kj 2CO(g) + O_2(g) rightarrow 2CO_2(g) delta H = -566 kJ 2CO_2(g) + 6H_2O(g) rightarrow 2C_2H_6(g) + 7O_2(g) delta H= +3122kJ

Explanation / Answer

intially both O3 and O2 are 0.1 mol and 0.1 mol

for 1 mole of O3 there should be a 3/2 mole of O2 accordingly

for 0.1 mol O3 there should be a 0.15 mole of O2

so in order to achieve the equilibrium

concentration of O3 should decrease and concentration of O2 should increase

option B is correct answer

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