2015年4月21日 · The relationship is: DeltaG^(0)=-RTlnK R is the gas constant = 8.31"J/K""/""mol" T is the absolute temperature K is the equilibrium constant Large values of K result in negative values of DeltaG indicating reaction spontaneity.

2014年5月28日 · By definition delta G is going to be the same as delta Go under standard conditions. dG isn't going to equal zero under standard conditions (because dGo would be zero too), but the equation dGo = -RTlnK assumes the reaction is in equilibrium I think (note we are using K and not Q), which is why dG=O.

2010年8月10日 · 1. delta Gnot is the Gibbs free energy in standard conditions. Those are the conditions where you use the formula -RTlnKeq. delta G on the other hand is the gibbs free energy at any given time, given the current ratio of products to reactants.

2015年9月12日 · Every reaction in a closed system is in some sort of equilibrium. Depending on the equilibrium constant K or its variants (K_a, K_b, K_"sp", etc), the equilibrium is skewed to a certain extent towards either the products or reactants. A common type of equilibrium is found in acid/base reactions. For acids and bases, there is a specific equation you can use to determine the extent of this ...

2009年4月25日 · the equation deltaG=-RTlnK just relates standard deltaG to the equilibrium constant, using R constant and Temp. to get from standard deltaG to just any delta G (meaning delta G at a different set of conditons other than 25C and 1atm and where all concentrations are 1M), you need to use the equation:

2018年4月25日 · Well, the standard change in Gibbs' free energy of reaction, DeltaG_(rxn)^@ can be found at equilibrium since you have K. This is for the reaction "AgI"(s) rightleftharpoons "Ag"^(+)(aq) + "I"^(-)(aq) You have this equation from your notes: DeltaG = DeltaG^@ + RTlnQ At equilibrium, DeltaG = 0 and Q = K. Therefore, DeltaG^@ = -RTlnK For dissolution of solids in water, K -= K_(sp). As a result ...

2017年8月12日 · If we know the equilibrium constant, K_(eq), for a chemical change we can calculate the standard state free energy change, Delta G^@. The "free energy" change for a reaction may determine whether it will be spontaneous or not, but "equilibrium" is just the final state of a system. The equations may be solved either way, depending on the available data (equilibrium concentrations or energy ...

2017年6月26日 · Negative values of DeltaG denote a "spontaneous reaction". If DeltaG=0, then the reaction is at equilibrium. And if DeltaG>0 then the reaction is non-spontaneous.... DeltaG may also be related to the equilibrium constant, K_"eq" by the equation: DeltaG^@ =-RTlnK_"eq".

2016年10月9日 · An enthalpy term and an entropy term. DeltaG^@=DeltaH^@ -TDeltaS^@ The Gibbs free energy is the single, unequivocal criterion for the spontaneity of chemical change. Negative values of DeltaG denote a "spontaneous reaction". DeltaG may also be related to the equilibrium constant, K_"eq" by the equation: DeltaG^@ =-RTlnK_"eq".

2017年7月18日 · You'd start from the expression for the change in Gibbs' free energy, DeltaG, relative to a reference, DeltaG^@, at standard pressure and a convenient temperature: DeltaG = DeltaG^@ + RTlnQ where: Q is the reaction quotient for the current state of the reaction. R and T are known from the ideal gas law. RTlnQ describes the shift in the free energy in reference to standard pressure and the ...