Open Question
At 45 °C, Kc = 0.619 for the reaction N2O4(g) ⇌ 2 NO2(g). If 46.0 g of N2O4 is introduced into an empty 2.00-L container, what are the partial pressures of NO2 and N2O4 after equilibrium has been achieved at 45 °C?
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 116
Calculate the equilibrium concentrations of SO2, Cl2, and SO2Cl2 at 298 K if the initial concentrations are [SO2] = 1.50 M and [Cl2] = 0.85 M. The equilibrium constant Kc for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g) is 8.40 × 10^-3 at 298 K.
Verified step by step guidance1
Write the balanced chemical equation for the reaction: \( \text{SO}_2(g) + \text{Cl}_2(g) \rightleftharpoons \text{SO}_2\text{Cl}_2(g) \).
Define the initial concentrations: \([\text{SO}_2] = 1.50 \text{ M}\), \([\text{Cl}_2] = 0.85 \text{ M}\), and \([\text{SO}_2\text{Cl}_2] = 0 \text{ M}\).
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in concentrations as the system reaches equilibrium.
Express the changes in concentration in terms of \(x\), where \(x\) is the amount of \(\text{SO}_2\text{Cl}_2\) formed at equilibrium. The changes will be: \([-x]\) for \(\text{SO}_2\) and \(\text{Cl}_2\), and \([+x]\) for \(\text{SO}_2\text{Cl}_2\).
Write the expression for the equilibrium constant \(K_c = \frac{[\text{SO}_2\text{Cl}_2]}{[\text{SO}_2][\text{Cl}_2]}\) and substitute the equilibrium concentrations from the ICE table into this expression to solve for \(x\).
Related Practice
Open Question
When 9.25 g of ClF3 was introduced into an empty 2.00-L container at 700.0 K, 19.8% of the ClF3 decomposed to give an equilibrium mixture of ClF3, ClF, and F2. ClF3 (g) ⇌ ClF (g) + F2 (g). (a) What is the value of the equilibrium constant Kc at 700.0 K? (b) What is the value of the equilibrium constant Kp at 700.0 K? (c) In a separate experiment, 39.4 g of ClF3 was introduced into an empty 2.00-L container at 700.0 K. What are the concentrations of ClF3, ClF, and F2 when the mixture reaches equilibrium?
Textbook Question
The reaction of fumarate with water to form L-malate is catalyzed by the enzyme fumarase; Kc = 3.3 at 37°C. When a reaction mixture with [fumarate] = 1.56 * 10-3 M and [l -malate] = 2.27 * 10-3 M comes to equilibrium in the presence of fumarase at 37 °C, what are the equilibrium concentrations of fumarate and L-malate? (Water can be omit- ted from the equilibrium equation because its concentration in dilute solutions is essentially the same as that in pure water.)
834
views
Open Question
Calculate the equilibrium concentrations of H2O(g), Cl2(g), HCl(g), and O2(g) at 298 K if the initial concentrations are [H2O] = 0.050 M and [Cl2] = 0.100 M. The equilibrium constant Kc for the reaction H2O(g) + Cl2(g) ⇌ 2 HCl(g) + O2(g) is 8.96 × 10^-9 at 298 K.
Textbook Question
Consider the following equilibrium: Ag+ (aq) + Cl-(aq) → AgCl(s) Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (c) Adding NO3, which reacts with Ag+ to form the complex ion Ag(NH3)2+
331
views
Textbook Question
Consider the following equilibrium: Ag+(aq) + Cl-(aq) ⇌ AgCl(s) Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (d) Removing Cl-; also account for the change using the reaction quotient Qc
350
views