The value of Keq for the following reaction is 0.25:
SO2 (g) + NO2 (g)<~> SO3 (g) + NO (g)
The value of Keq at the same temperature for the reaction below is __________.
2SO2 (g) + 2NO2 (g)<~> 2SO3 (g) + 2NO (g)
answer is 0.25 how do i figure this out?
The rules for Keq are clear: the exponents used must be from the balanced equation, and we specify a standard for balancing as the lowest whole number ratio.
Balanced:
Ba + F2> BaF2
C+ 2H2 + 2O2 >> CO2 + 2H20
NOT C + H2+3/2 O2 >> CO2 + H2O
To determine the value of Keq for the second reaction, you need to understand the relationship between the equilibrium constants (Keq) and the stoichiometric coefficients of the balanced equation.
The balanced equation for the first reaction is:
SO2 (g) + NO2 (g) <~> SO3 (g) + NO (g)
The equilibrium constant expression (Keq) for this reaction can be written as:
Keq = [SO3][NO] / [SO2][NO2]
Given that the value of Keq for the first reaction is 0.25, you have:
0.25 = [SO3][NO] / [SO2][NO2]
Now, let's examine the balanced equation for the second reaction:
2SO2 (g) + 2NO2 (g) <~> 2SO3 (g) + 2NO (g)
Notice that all stoichiometric coefficients have been doubled compared to the first reaction. Therefore, the equilibrium constant expression (Keq) for the second reaction is:
Keq = [SO3]^2[NO]^2 / [SO2]^2[NO2]^2
Since the stoichiometric coefficients are squared, the value of Keq for the second reaction will be the square of the value of Keq for the first reaction:
Keq (second reaction) = (Keq first reaction)^2
Keq (second reaction) = (0.25)^2
Keq (second reaction) = 0.0625
Hence, the value of Keq at the same temperature for the second reaction is 0.0625.
To calculate the value of Keq for the given reaction, you need to use the balanced equation and the concentrations of the reactants and products.
Given reaction: SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g)
The reaction equation shows that the stoichiometric coefficients of the reactants and products are 1. This means that there is a 1:1 ratio between the reactants and products.
The expression for Keq is given by:
Keq = [products] / [reactants]
In this case, the Keq value is given as 0.25, which means that at equilibrium, the concentration of products is one-fourth (0.25) of the concentration of reactants.
Now, let's calculate the value of Keq for the second reaction:
2SO2 (g) + 2NO2 (g) <=> 2SO3 (g) + 2NO (g)
Since the stoichiometric coefficients in this reaction are 2, the concentrations of reactants and products will be double (2:1 ratio) compared to the first reaction.
Therefore, the concentration of products in the second reaction will be double, and the concentration of reactants will be the same.
Using the given Keq value (0.25) from the first reaction, we can find the new Keq value for the second reaction.
Keq (second reaction) = (concentration of products) / (concentration of reactants)
Since the concentration of products in the second reaction is twice that of the first reaction, and the concentration of reactants is the same:
Keq (second reaction) = (2 * 0.25) / 1 = 0.5
Thus, the value of Keq at the same temperature for the second reaction is 0.5.