A level chemistry equilibrium
N2 + 3H2 = 2NH3. The pressure exerted by these gases at constant temperature is 2.000 x 10^7 Pa. Under these conditions, partial pressure of N2 and H2 is 1.490 x 10^7 Pa and 0.400 x 10^7 Pa respectively. Calculate the value of Kp for this reaction. Im completely lost.
I've not done this sort of problem before but...
You have the total pressure. This is the sum of the partial pressure. You can use this to work out the partial pressure of ammonia
Kp like other equilibrium constants is products/reactants
You have the total pressure. This is the sum of the partial pressure. You can use this to work out the partial pressure of ammonia
Kp like other equilibrium constants is products/reactants
Original post by mocha520
N2 + 3H2 = 2NH3. The pressure exerted by these gases at constant temperature is 2.000 x 10^7 Pa. Under these conditions, partial pressure of N2 and H2 is 1.490 x 10^7 Pa and 0.400 x 10^7 Pa respectively. Calculate the value of Kp for this reaction. Im completely lost.
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