What is the significance of a very large Kp value on the equilibrium concentration of H2 in the reaction : 2H2 (g) + O2 (g) <-> 2H2O (g) ?
A. There is very little H2 at equilibrium.
B. There is a significant amount of H2 at equilibrium.
C. The amount of H2 does not depend on the value of Kp
D. The amount of H2 is always equal to the amount of O2 at equilibrium.
I am pretty sure that the answer has to be either A or B as C and D don't really make sense. Can someone please help me out?
So the answer is A
yes. There will relatively large amount of H2O and relatively small amounts of H2 and O2 at equilibrium when Kp is large. The reverse is true when you have a small value for Kp. Have you studied Ksp yet? For solubility product, the numbers tell you how soluble a substance is. For example, AgCl has a Ksp of about 1E-10. AgCl(solid) ==> Ag^+(aq) + Cl^-(aq)
So Ksp expression is 1E-10 = (Ag^+)(Cl^-). With a number small like 1E-10 you know that AgCl is sparingly soluble and it takes little to form a saturated solution of AgCl.
You're right. Neither C nor D are correct. So now you're down to guessing for A or B. But why guess? Write the Kp expression.
Kp = very large = p^2(H2O)/p^2(H2)*p(O2)
To get a very large number in ANY fraction you must have either a large numerator OR a very small denominator (or both). Now, shouldn't that tell you the there must be a bunch of products (the numerator) and a very small amount of reactants (the denominator)? Now you can answer the question. I just gave you the answer.
Thank you DrBob222
To understand the significance of a very large Kp value on the equilibrium concentration of H2 in the given reaction (2H2 (g) + O2 (g) <-> 2H2O (g)), we need to understand the concept of Kp.
Kp is the equilibrium constant in terms of partial pressures and represents the ratio of the products of the concentrations of the products to the products of the concentrations of the reactants, each raised to the power of their stoichiometric coefficients. In this case, the value of Kp will be determined by the concentrations of H2, O2, and H2O at equilibrium.
A large Kp value indicates that the products (H2O) are favored at equilibrium, while a small Kp value indicates that the reactants (H2 and O2) are favored.
Now, let's analyze the answer choices:
A. There is very little H2 at equilibrium.
- This option suggests that H2 is not favored at equilibrium. However, a large Kp value indicates that the products are favored, so this option is incorrect.
B. There is a significant amount of H2 at equilibrium.
- This option suggests that H2 is favored at equilibrium, which is consistent with a large Kp value. Therefore, this option is likely to be the correct answer.
C. The amount of H2 does not depend on the value of Kp.
- This option is incorrect because the value of Kp directly affects the concentration of H2 at equilibrium.
D. The amount of H2 is always equal to the amount of O2 at equilibrium.
- This option is incorrect as the stoichiometry of the reaction shows that there are twice as many H2 molecules as O2 molecules in the balanced equation.
Based on our analysis, it is likely that the correct answer is option B: There is a significant amount of H2 at equilibrium.