## Example 5I.4

Paige Lee 1A
Posts: 136
Joined: Sat Sep 07, 2019 12:16 am

### Example 5I.4

For this example, how do you know to find the partial pressures and not the concentrations at equilibrium?

Zaynab Hashm 2I
Posts: 110
Joined: Wed Sep 11, 2019 12:15 am
Been upvoted: 1 time

### Re: Example 5I.4

If you mean why we have to use partial pressure, it's because the question mentions that they're in a gas-phase equilibrium. We use partial pressure for gases.

Alex Tchekanov Dis 2k
Posts: 118
Joined: Sat Aug 24, 2019 12:16 am

### Re: Example 5I.4

If you want to convert from concentration to partial pressure you have to use the ideal gas law: PV=nRT
P=(n/V)RT
P=ConcRT
Cont=P/RT

Pegah Nasseri 1K
Posts: 100
Joined: Wed Feb 27, 2019 12:15 am

### Re: Example 5I.4

Always when calculating K for gases, partial pressure is used. However, if the question specifically asks you to find then you would use the concentration of the gases. You would convert the partial pressure of the gases to molar concentration using the equation PV=nRT (n/V (concentration) = P/RT).

705302428
Posts: 50
Joined: Sat Aug 24, 2019 12:16 am

### Re: Example 5I.4

Because we use partial pressure when dealing with gasses.