00:01
To determine the equilibrium partial pressures of no and o2, we'll start with our balanced chemical reaction.
00:10
2n02 decomposes into 2no and o2.
00:16
Kp is going to be equal to the pressure of no squared because it's coefficient as 2, multiplied by the pressure of o2, divided by the pressure of no2 squared, and they tell us that that value is 4 .48 times 10 to the negative 13.
00:47
So if we initially start with a pressure of 0 .55 atmospheres of n0 and nothing of n0 or 0, then after a change occurs, this decreasing by 2x, this increasing by 2x, and this increasing by x, following their coefficients.
01:16
Then we'll have 0 .55 minus 2x, 2x, 2x, and x at equilibrium.
01:28
So going back to our kp expression, kp equals 4 .48 times 10 to the negative 13, and that, will be equal to the pressure of no 2x squared multiplied by the pressure of 02 x divided by the pressure of no2 because this kp value is so small 2x should be negligible in comparison to 0 .55 so we can remove that and just put 0 .55 down here which is commonly done with very small k values...