It is spontaneous at 2000 K.
Toward I2(s) production
430k
430 K
Toward I2(s) production
2SO2(g) + O2(g) 2SO3(g)-The reverse reaction is favored.
Toward I2(s) production
Gas phase Iodine in open cylinder
I2(s) --> I2(g); dH=62.4kJ/mol; dS=0.145kJ/mol. The reaction will favor the product at this temperature. Your entropy is positive and your enthalpy is also positive, so this reaction will not be spontaneous at all temperatures. But at room temperature, which is 298K, it will be spontaneous and proceed left to right. (this is the sublimation of iodine)
products are favored over reactants in the reaction.
Toward I2(s) production
2SO2(g) + O2(g) 2SO3(g)-The reverse reaction is favored.
Toward I2(s) production
This is False!!! According to LeChatlier's Principle, increasing the temperature is a strees on the equilibrium. To relieve that stress the reaction will shift producing more of the substances on the side of the reaction that absorbs heat energy.
Gas phase Iodine in open cylinder
I2(s) --> I2(g); dH=62.4kJ/mol; dS=0.145kJ/mol. The reaction will favor the product at this temperature. Your entropy is positive and your enthalpy is also positive, so this reaction will not be spontaneous at all temperatures. But at room temperature, which is 298K, it will be spontaneous and proceed left to right. (this is the sublimation of iodine)
products are favored over reactants in the reaction.
reactants are favored over products in the reaction
If all the reactants occupy more volume than all of the products, the reverse reaction will be favored. If all the reactants occupy less volume than all of the products, the forward reaction will be favored. If the products and reagents have the same volume, the equilibrium will not change.
product and reaction are equality favored in the reaction
the forwrd reaction is favored
products are favored over reactants in the reaction.