Skip to main content
Pearson+ LogoPearson+ Logo
Ch.15 - Chemical Equilibrium
All textbooksMcMurry 8th EditionCh.15 - Chemical EquilibriumProblem 108
Previous problem
Next problem
Chapter 15, Problem 108

At 500 °C, F2 gas is stable and does not dissociate, but at 840 °C, some dissociation occurs: F2(g) ⇌ 2 F(g). A flask filled with 0.600 atm of F2 at 500 °C was heated to 840 °C, and the pressure at equilibrium was measured to be 0.984 atm. What is the equilibrium constant Kp for the dissociation of F2 gas at 840 °C?

Verified step by step guidance
1
Step 1: Write the balanced chemical equation for the dissociation of F2: F2(g) ⇌ 2 F(g).
Step 2: Define the initial pressure of F2 and the change in pressure due to dissociation. Initially, the pressure of F2 is 0.600 atm.
Step 3: Let x be the change in pressure of F2 that dissociates. At equilibrium, the pressure of F2 will be (0.600 - x) atm, and the pressure of F will be 2x atm.
Step 4: Use the total pressure at equilibrium (0.984 atm) to set up the equation: (0.600 - x) + 2x = 0.984.
Step 5: Solve for x to find the equilibrium pressures of F2 and F, then use these pressures to calculate the equilibrium constant Kp using the expression Kp = (P_F)^2 / (P_F2).
Previous problem
Next problem
Related Practice
Open Question
The equilibrium constant Kp for the gas-phase thermal decomposition of tert-butyl chloride is 3.45 at 500 K: CH3C(CH3)2Cl(g) ↔ CH2=C(CH3)2(g) + HCl(g). (b) Calculate the molar concentrations of reactants and products in an equilibrium mixture obtained by heating 1.00 mol of tert-butyl chloride in a 5.00-L vessel at 500 K. (c) A mixture of isobutylene (0.400 atm partial pressure at 500 K) and HCl (0.600 atm partial pressure at 500 K) is allowed to reach equilibrium at 500 K. What are the equilibrium partial pressures of tert-butyl chloride, isobutylene, and HCl?
Textbook Question
At 100 °C, Kc = 4.72 for the reaction 2 NO21g2 ∆ N2O41g2. An empty 10.0-L flask is filled with 4.60 g of NO2 at 100 °C. What is the total pressure in the flask at equilibrium?
728
views
Open Question
At 25 °C, Kc = 216 for the reaction 2 NO2(g) ⇌ N2O4(g). A 1.00-L flask containing a mixture of NO2 and N2O4 at 25 °C has a total pressure of 1.50 atm. What is the partial pressure of each gas?
Open Question
The reaction NO(g) + NO2(g) ⇌ N2O3(g) takes place in the atmosphere with Kc = 13 at 298 K. A gas mixture is prepared with 2.0 mol NO and 3.0 mol NO2 and an initial total pressure of 1.65 atm. (a) What are the equilibrium partial pressures of NO, NO2, and N2O3 at 298 K?
Textbook Question
The equilibrium constant Kc for the reaction N21g2 + 3 H21g2 ∆ 2 NH31g2 is 4.20 at 600 K. When a quantity of gaseous NH3 was placed in a 1.00-L reaction vessel at 600 K and the reaction was allowed to reach equilibrium, the vessel was found to contain 0.200 mol of N2. How many moles of NH3 were placed in the vessel?
432
views
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?