Keq=[H2][Cl2]/[HCl]2
keq=[SO3]2[O2] [So3]2
Molarity of products divided by reactants Keq=(products)/(reactants)
For 2HCl(g) ==> H2(g) + Cl2(g) the Keq = [H2][Cl2]/[HCl]^2
The reaction quotient is the ratio of products to reactants not at equilibrium. If the system is at equilibrium then Q becomes Keq the equilibrium constant. Q = products/reactants If Q < Keq then there are more reactants then products so the system must shift toward the products to achieve equilibrium. If Q > Keq then there are more products than reactants and the system must shift toward the reactants to reach equilibrium.
SO2(g) + NO2(g) ==> SO3(g) + NO(g)Keq = [SO3][NO]/[SO2][NO2] Without knowing concentrations, one cannot calculate the actual value of Keq.
Keq = [H2O][CO] [H2][CO2]
HI will be consumed. The reaction will proceed to the left. More I2 will form.
Changing the temperature will change Keq. (apex.)
Products. keq equals [products] / [reactants] . A (-) Keq indicates a reactant favored reaction.
K(eq)= 1.33
Keq=[H2][Cl2]/[hcl]^2
keq=[SO3]2[O2] [So3]2
Changing the temperature will change Keq - apex (Explanation): Keq is closely related to temperature and is part of the equation, so changing temperature will change Keq. Temperature does speed up the reaction sometimes, but that is not the only thing that it can affect.
Products and reactions are equally favored in the reactions
keq= [SO2]2[O2]/[SO3]2
If a reaction creates far more products than reactants, the numerator is large and the denominator is small. That means Keq will be large. So when Keq is large, equilibrium is to the far right of the reaction. A reaction that goes to completion would have an infinite Keq, since the concentration of reactants goes all the way to zero.If few products form, and many reactants remain, the numerator is small and the denominator is large. So a small Keq means that equilibrium is far to the left.you're welcome.
products are favored over reactants in the reaction.