Answer:
Equilibrium constant is 0.0873
Explanation:
For the reaction:
A + B ⇄ C
Equilibrium constant is defined as:
K = [C] / [A] [B]
concentrations in equilibrium of each reactant are:
[A] = 10 - X
[B] = 5 - X
[C] = 15 + X
If concentration in equilibrium of B is 9, X is:
[B] = 5 - X = 9 → <em>X = -4 </em>
Replacing:
[A] = 10 - (-4) = 14
[B] = 5 - (-4) = 9
[C] = 15 + (-4) = 11
K = 11 / (14×9) = 0.0873
Thus, <em>equilibrium constant is 0.0873</em>
Answer:
The average atomic mass of oxygen is 15.999u
The rate constants, K, can be expressed in many different terms. In this case, Kp is the equilibrium constant expressed in terms of gas partial pressure. The formula for this is:
Kp = [P(product C) × P(product D)] / [P(reactant A) × P(reactant B)]
As there is only one product, we will use only its pressure in the numerator.
Kp = [P(COCl2)] / [P(CO) × P(Cl2)]
P(COCl2) = 1.49 × 10⁸ × 2.22 × 10⁻⁴ × 2.22 × 10⁻⁴
P(COCl2) = 7.34 atm
