Nitric oxide (NO) reacts with molecular oxygen as follows:
2NO(g) + O2(g) �¨ 2NO2(g)
Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and calculate their partial pressures. Assume that the temperatures remains constant at 25 Celsius.
Calculate the partial pressure of NO, O2 and NO2.
Volume of NO= 4.00L
Pressure of No= 0.500atm
Pressure of O2= 1.97 atm
Volume of O2 = 1.00 L
1 answer
if equilibrium partial pressure of n2, o2 and no are respectively at 2200 degrees C, what is kp?