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Ch.15 - Chemical Equilibrium
All textbooksMcMurry 8th EditionCh.15 - Chemical EquilibriumProblem 107
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Chapter 15, Problem 107

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?

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1
Step 1: Use the ideal gas law to relate the total pressure to the concentrations of NO2 and N2O4. Since the volume and temperature are constant, the partial pressures can be related to the concentrations by P = nRT/V.
Step 2: Express the equilibrium constant Kc in terms of partial pressures. For the reaction 2 NO2(g) ⇌ N2O4(g), Kc = [N2O4]/[NO2]^2. Convert this to Kp using the relation Kp = Kc(RT)^Δn, where Δn is the change in moles of gas.
Step 3: Set up the expression for the total pressure in terms of the partial pressures: P_total = P_NO2 + P_N2O4. Use the stoichiometry of the reaction to express the partial pressures in terms of a single variable, such as the change in moles of NO2.
Step 4: Substitute the expressions for the partial pressures into the equilibrium expression for Kp. Solve the resulting equation for the variable representing the change in moles of NO2.
Step 5: Calculate the partial pressures of NO2 and N2O4 using the solved value from Step 4 and the total pressure equation.
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Related Practice
Open Question
15.104 Consider the reaction C(s) + CO2(g) ⇌ 2 CO(g). When 1.50 mol of CO2 and an excess of solid carbon are heated in a 20.0-L container at 1100 K, the equilibrium concentration of CO is 7.00 x 10^-2 M. (a) What is the equilibrium concentration of CO2? (b) What is the value of the equilibrium constant Kc at 1100 K?
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?
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Textbook Question
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