the eqilibrium constant is apparently only affected by temperature. surely though by definition pressure affects it also (PV/T=a constant). can someone explain?
2006-11-07 05:24:49 · 3 answers · asked by vvv 1 in Science & Mathematics ➔ Chemistry
It is also affected by pressure only if one of the constituents is a gas.
2006-11-07 05:48:31 · answer #1 · answered by ag_iitkgp 7 · 0⤊ 0⤋
Pressure times volume divided by Temperature in a closed system will remain a constant. The ideal gas law PV=nrT where P is the pressure in mm of Hg, V is the volume, T is the temperature in degrees Kelvin, n is the number of moles of gas present and r is the gas constant. In a closed system, the number of atoms of gas will not change and r is already a constant. Basically it says that if the pressure goes up, either the temperature goes up, or the volume goes down, or a combination thereof and if the pressure goes down, the temperature goes down or the volume goe up, or a combination again.
2006-11-07 13:38:30 · answer #2 · answered by SteveA8 6 · 0⤊ 0⤋
The equilibrium constant is a constant- it does not change with P, V or T for stable gases. However, any change in gas composition by reactions or otherwise can have an impact
2006-11-08 09:19:40 · answer #3 · answered by kapilbansalagra 4 · 0⤊ 0⤋