Consider the reaction 2 NO (g) + O 2 (g) 2NO 2 (g) At a given temperature, an eq

Question

Consider the reaction              2 NO (g) + O2(g) 2NO2(g) At a given temperature, an equilibrium mixture consists of0.020 moles of O2 , 0.040 moles of NO, and 0.96moles of NO2. The total gas pressure ( NO, O2and NO2 ) is 0.20 atm. Calculate Kp for thisreaction. hint: Remember Dalton's law of partial pressures. Consider the reaction              2 NO (g) + O2(g) 2NO2(g) At a given temperature, an equilibrium mixture consists of0.020 moles of O2 , 0.040 moles of NO, and 0.96moles of NO2. The total gas pressure ( NO, O2and NO2 ) is 0.20 atm. Calculate Kp for thisreaction. hint: Remember Dalton's law of partial pressures.

Explanation / Answer

According to Dalton's theory Total pressure = PO2 +PNO + PNO2    We have the total pressure = 0.20 atm Total moles of the mixture = 0.020 + 0.040 + 0.96= 1.02 mole mole fraction of Oxygen = 0.020/1.02 =0.019     partial pressure of the oxygen in themixture = total pressure * mole fraction                                                                      = 0.20 * 0.019                                                                      = 0.003921 atm Similarly the partial pressure of theNO    = 0.20 * (0.040/1.02)                                                                = 0.00784 atm partial pressure of theNO2                     = 0.20 * (0.96/1.02)                                                                = 0.1882 Therefore for the reaction                                        2 NO (g) + O2(g) 2NO2(g)           Kp = PNO22 / PNO2* PO2                   =(0.188)2 /(0.00784)2*0.003921                  = 1.47*105                   =(0.188)2 /(0.00784)2*0.003921                  = 1.47*105

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