Learning Goal: To determine equilibrium concentrations from initial conditions.

Question

Learning Goal:

To determine equilibrium concentrations from initial conditions.

The reversible reaction

XY(aq)X(aq)+Y(aq)

has a reaction quotient Qc defined as

Qc=[X][Y][XY]

Because the reaction is reversible, both the forward and reverse reactions will occur simultaneously. The reaction will eventually reach equilibrium, at which point the concentrations do not change, and Qc is equal to a constant known as Kc.

Part C

Based on a Kc value of 0.180 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

MasteringChemistry: RCT #8 Chemical Equilibrium (Qc/Qp and Le Chatelier&#x2019 s Principle pp. 653 683-Google Chrome Secure l https://session.masteringchemistry.com/myct/itemView?assignmentProblemID=95453464 RCT #8 Chemical Equilibrium (Qc/Qp and Le Chatelier’s Principle) pp.653-683 ± Fundamentals of Equilibrium Concentration Calculations 7 of 14 Concentration (M) XY 0.200 TY 0.300 The reversible reaction 0.300 XY(aq)X(a) Y(aq) has a reaction quotient Qc defined as equilibrium 0.200 z 0.300-z 0.300- The change in concentration, z, is positive for the reactants because they are produced and negative for the products because they are consumed ec Because the reaction is reversible, both the forward and reverse reactions will occur simultaneously. The reaction will eventually reach equilibrium, at which point the concentrations do not change, and is equal to a constant known as Ko Part C Based on a Ke value of 0.180 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively'? Express the molar concentrations numerically. View Available Hint(s) Figure 1 of 1 K Q incorrect; One attempt remaining: Try Again Term 1: Not quite. Check through your calculations; you may have made a rounding error or used the wrong number of significant figures Reacton forms products Reacton forms reactants Equilibnnum Provide Feedback Next > S17 PM O Type here to search

Explanation / Answer

We can simply write Kc = [X][Y] / [XY]

put the values given in table at equillibirium:

0.18 = (0.300- x)* (0.300- x) / (0.200 +x)

0.18* (0.200 +x) = (0.300- x)* (0.300- x)

0.036 + 0.18x = 0.09 + x2 - 0.6x

x2 - 0.78x + 0.054 =0

x = 0.076

So [X] = 0.300- x = 0.300 - 0.076 = 0.224 M

[X] = [Y] = 0.224 M

[XY] = 0.200 + x = 0.200 + 0.076 = 0.276 M

Related Questions

Navigate

• Browse (All)
• Browse L
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.