Chem Kp Question help
In the following reaction at 700K, the amount of each gas present at equilibrium is 0.960 moles of NO2, 0.040 moles of NO, and 0.020 moles of O2.
If Kp = 6.8 (x 10 ^-6) atm, what must the total pressure have been to achieve this particular equilibrium mixture?
2 NO2(g) -------> 2 NO(g) + O2(g)
If Kp = 6.8 (x 10 ^-6) atm, what must the total pressure have been to achieve this particular equilibrium mixture?
2 NO2(g) -------> 2 NO(g) + O2(g)
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