Partial Pressures

[kate cassiano 1F]

Can someone explain to me out to calculate partial pressures when asked in a chemical equilibrium question?

[Joshua Chandran 2D]

If we are given a chemical equilibrium problem that has all gases, we most likely would need to set up an ICE table and use a given Kp value to find equilibrium partial pressures. If the question asks to find the partial pressure of a compound from its concentration, we would have to use the ideal gas equation, PV = nRT, in which P=partial pressure, V = volume, n=number of moles, R=ideal gas constant, and T=temperature in Kelvin. We could rearrange this equation so P = (n/v)RT = concentration(RT) to find the partial pressure.

[Linette Ocegueda 3D]

If we are given Kc and we need to find Kp In atm we can also do kc(RT)^delta n

Where kc: equilibrium concentration
R: 0.0821 in atm
T: temperature
Delta n: will be difference in moles from products and reactants and the way to calculate/ find delta n will be # of moles for products - # of moles for reactants