00:01
In this problem, 1 mole of n204 at 310 kelvin is 25 % dissociated at 1 atmospheric pressure.
00:12
So n2 -2 -2 -10 gas decomposes to give 2 moles of no2 at 310 kelvin.
00:31
Initial moles of n -2 is equal to 1 and no2 is 0.
00:48
At equilibrium, n -204 is decreased by alpha and no2 is increased by 2 alpha where alpha indicates percentage dissociation.
01:26
Now total moles at equilibrium is equal to 1 minus alpha plus 2 alpha so we get total mole equals to 1 plus alpha.
01:51
We can write kp is equal to partial pressure of no2 raise to the power 2, divide 2, by partial pressure of n2o4.
02:12
So partial pressure of no2 is equal to total pressure p into mole fraction of no2 raise to the power 2 and partial pressure of n2 is equal to total pressure p into mole fraction of n2 4.
02:34
Here p indicates total pressure at equilibrium.
02:55
So we can write p squared into mole fraction of no2 is equal to moles of no2 divide by total moles and more fraction of n -2 of 4 is equal to 1 minus alpha divide by 1 plus alpha.
03:20
So we get kp is equal to 4p alpha squared by 4p alpha squared by 1 minus alpha square so we get kp equals to 4p alpha square divide by 1 minus alpha square by rearranging this expression we get alpha is equal to kp divide by 4p plus kp raised to the power 1 half now we have given alpha is equal to 0 .2 5 and pressure p is equal to 1 atm...