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)
3600 k - apex
It tells whether products or reactants are favored at equilibrium
Toward I2(s) production
2SO2(g) + O2(g) 2SO3(g)-The reverse reaction is favored.
Gas phase Iodine in open cylinder
products are favored over reactants in the reaction.
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.
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.
It tells whether products or reactants are favored at equilibrium
the forwrd reaction is favored
It tells whether products or reactants are favored at equilibrium
Forward reaction favored, concentration of products is higher
Toward I2(s) production
Products and reactions are equally favored in the reactions
equilibrium will shift to the side of the equation with the least moles in attempt to reduce pressure in the haber process N2+3H2 <--> 2NH3 an increase in pressure causes equilibrium to shift the right because it has the least moles (2 instead of 4) <--> represents a reversible reaction sign
Toward I2(s) production
2SO2(g) + O2(g) 2SO3(g)-The reverse reaction is favored.
It tells how much the reaction rate is affected by concentrations.