partial pressures and Kp
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what is the partial pressure of a gas in a mixture?
the pressure that the gas would have if it alone occupied the volume occupied by the whole mixture if a mixture of gases contains 3 different gases then the total pressure will equal the 3 partial pressures added together P = p1 + p2 + p3
what is the mole fraction equation?
number of moles of a gas/ total number of moles of all gases
what is the equation for partial pressure of a gas ?
mole fraction of that gas x total pressure
how do we write an expression for Kp?
Kp= equilibrium constant p= partial pressure of that gas Kp= partial pressure of gaseous products / partial pressure of gaseous reactants use co-efficients as powers just like Kc
what do we only use in the Kp equation and what brackets?
only include gases, ignore solids, liquids, and aqueous substances use curved brackets and NOT square as this is not concentration!!!
how do we work out the units of Kp?
units of pressure kPa are used and then cancel out units just like when doing Kc
what does it mean if Kp is larger/ smaller?
larger means greater amount of products smaller means equilibrium favours reactants
what does Kc and Kp change with/ not change with?
only with temp they do not change is pressure or concentration are altered, also not in presence of catalyst
what changes when temp changes?
position of equilibrium and therefore Kp