It is spontaneous at 2000 K.
Toward I2(s) production
430k
430 K
The reaction is favored in the forward direction at 298 K (room temperature) because it is an exothermic reaction. The negative enthalpy change (-62.4 kJ/mol) indicates that energy is released in the forward reaction. This, combined with the positive entropy change (S = 0.145 kJ/molK), suggests that the disorder of the system increases as the reaction proceeds in the forward direction, making it more favorable at room temperature.
Toward I2(s) production
Toward I2(s) production
Gas phase Iodine in open cylinder
Raising the temperature of a chemical reaction typically increases the rate of the reaction as it provides more energy for the molecules to react. This is because a higher temperature increases the kinetic energy of molecules, allowing them to collide more frequently and with greater force, leading to more successful collisions and faster reaction rates.
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
Raising the temperature of a chemical reaction typically increases the rate of the reaction as it provides more energy for the molecules to react. This is because a higher temperature increases the kinetic energy of molecules, allowing them to collide more frequently and with greater force, leading to more successful collisions and faster reaction rates.
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.