Consider the equilibrium of water with gaseous hydrogen and oxygen:
Give the value of for this reaction, if it is written as:
Choose one answer.
a. -7.8 x 10^-16
b. -3.9 x 10^-16
c. 1.3 x 10^-15
d. 6.4 x 10^-14
e. 3.6 x 10^2
give the value of WHAT for this reaction, ......
Consider the equilibrium of water with gaseous hydrogen and oxygen:
2H2O(g)=2H2(g) + O2(g) Kp= 7.8x10^-16
Give the value of for this reaction, if it is written as:
1/2O2(g) + H2(g) =H2O(g)
Choose one answer.
a. -7.8 x 10^16
b. -3.9 x 10^16
c. 1.3 x 10^15
d. 6.4 x 10^14
e. 3.6 x 10^7
You still didn't say "of what" but I assume it is Kp after you filled in th remainder of the missing information.
First you turned the reaction around. Let's designate the original Kp as Kp1. That makes the new Kp (which we will call Kp2) = 1/Kp1. THEN you divided all of the coefficients by 2. That makes Kp3 = sqrt(Kp2). Therefore, you take the reciprocal of the original Kp, then take the square root of that.
To determine the value of the equilibrium constant (K) for the reaction involving the equilibrium of water with gaseous hydrogen and oxygen, we need to write the balanced chemical equation and obtain the expression for K.
The balanced chemical equation for the reaction is:
2 H2(g) + O2(g) ⇌ 2 H2O(g)
The expression for K is given by the concentration of the products raised to their stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients.
K = [H2O]^2 / [H2]^2 [O2]
Since the reaction involves gases, we can use the partial pressure of the gases instead of their concentrations. Thus, the expression for K can be written in terms of partial pressures (P).
K = (P[H2O])^2 / (P[H2])^2 (P[O2])
However, to determine the value of K, we need additional information about the partial pressures of the gases at equilibrium. Without this information, it is not possible to calculate the exact value of K.
Therefore, based on the given options, it seems that none of the options provided is correct because they do not correspond to the correct value of the equilibrium constant for the given reaction.