Question

Rank the equilibrium constants for these three reactions from largest to smallest Rank from largest to smallest. To rank items as equivalent, overlap them

1. K(CI) 2. K(Br) 3. K(I2) Largest _____

Smallest ______

Answer 1

Without specific reactions or equilibrium constant values, we cannot rank the equilibrium constants for CI, Br, and I2. Equilibrium constants indicate reactant or product favorability; larger values suggest product preference. In titrations Kc > 1, and for gravimetric analysis, Ke > 1 is desired.

Step-by-step explanation:

To rank the equilibrium constants (K) for reactions involving chloride (Cl), bromide (Br), and iodine (I2), we need to consider the context in which these reactions occur or any provided equilibrium constant values. Unfortunately, without specific reactions or equilibrium constant values provided, we are unable to rank K(CI), K(Br), and K(I2) accurately. Moreover, the equilibrium constant can indicate the extent of a reaction; large K values (> 103) suggest the reaction favors products, whereas small K values (< 10-3) indicate a favor towards reactants. For titration reactions, Kc is typically > 1, for precipitation reactions useful in gravimetric analysis, Ke would be > 1, and for commercial processes like the conversion of acetylene to benzene, a higher K value is generally more desirable.

Answer 2

Answer: From largest to smallest

K(Cl) > K(Br) > K(I2)

Step-by-step explanation:

According to the first figure, two Cl2 molecules, two C2H4molecules, and eight C2H4Cl2 molecules are left. Using the law of mass action, you can find the equilibrium constant:

K= [C2H4Cl2]/ [C2H4][Cl2]=8/(2×2)=

K= 2

According to the second figure, four Br2molecules, four C2H4molecules, and six C2H4Br2 molecules are left. Using the law of mass action you can find the equilibrium constant:

K=[C2H4Br2]/[C2H4][Br2] =6/(4×4)=

K= 0.4

According to the third figure, seven I2 molecules, seven C2H4molecules, and three C2H4I2 molecules are left. Using the law of mass action you can find the equilibrium constant:

K=[C2H4I2]/ [C2H4][I2]= 3/(7×7)=

K= 0.06

Therefore, the equilibrium constant for Cl2 is the largest, and the equilibrium constant for I2 is the smallest, with Br2 falling in the middle of the two.