Consider the decomposition reaction shown below. NO2(g) ⇄ NO(g) + ½ O2(g) Temperature is 25 °C. ΔG°rxn is +34.85 kJ/mol Assuming the reaction takes place in a closed vessel with an initial NO2(g) pressure of 2.540 atm, what are the partial pressures of each of the gases at equilibrium? Show a complete ICE table. Indicate any assumptions that you made in your calculations.
Consider the decomposition reaction shown below. NO2(g) ⇄ NO(g) + ½ O2(g) Temperature is 25 °C. ΔG°rxn is +34.85 kJ/mol Assuming the reaction takes place in a closed vessel with an initial NO2(g) pressure of 2.540 atm, what are the partial pressures of each of the gases at equilibrium? Show a complete ICE table. Indicate any assumptions that you made in your calculations.
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Chapter18: Thermodynamics And Equilibrium
Section: Chapter Questions
Problem 18.124QP: Hydrogen gas and iodine gas react to form hydrogen iodide. If 0.500 mol H2 and 1.00 mol I2 are...
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Consider the decomposition reaction shown below.
NO2(g) ⇄ NO(g) + ½ O2(g)
Temperature is 25 °C. ΔG°rxn is +34.85 kJ/mol
Assuming the reaction takes place in a closed vessel with an initial NO2(g) pressure of 2.540 atm, what
are the partial pressures of each of the gases at equilibrium? Show a complete ICE table. Indicate any
assumptions that you made in your calculations.
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