Question 11
Marks: 4
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
You didn't finish the question. If written as what?
Sorry! Here it is: I am not sure where to start on this problem
Consider the equilibrium of water with gaseous hydrogen and oxygen: 2H2O ---2H2+O2
Kp =7.8*10^-16
Give the value of Kp for this reaction, if it is written as:
1/2 O2 +H2 ---H20
Choose following correct :
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
To find the value of K (equilibrium constant) for the reaction of water with gaseous hydrogen and oxygen, we need to consider the balanced equation and the definition of K.
The balanced equation for the reaction is:
2H2(g) + O2(g) ⇌ 2H2O(g)
The equilibrium constant expression (K) for this reaction is:
K = [H2O]^2 / [H2]^2 [O2]
In this equation, [H2O], [H2], and [O2] represent the concentrations of water, gaseous hydrogen, and gaseous oxygen, respectively.
To determine the value of K, we need to know the concentrations of the reactants and products at equilibrium. The information provided doesn't specify the concentrations, so we cannot calculate the exact value of K.
Therefore, without the specific concentrations, it is not possible to give the value of K. None of the options provided (a, b, c, d, e) are correct without the necessary data.