Consider the following equilibrium: N2O4(g)?2NO2(g) Thermodynamic data on these gases are given in Appendix C in...

Consider the following equilibrium:
N2O4(g)?2NO2(g)
Thermodynamic data on these gases are given in Appendix C in the textbook. You may assume that ?H? and ?S? do not vary with temperature.

Part A At what temperature will an equilibrium mixture contain equal amounts of the two gases? Express your answer using four significant figures

Part B

At what temperature will an equilibrium mixture of 1 atm total pressure contain twice as much NO2 as N2O4?

Express your answer using four significant figures.

Part C

At what temperature will an equilibrium mixture of 9 atm total pressure contain twice as much NO2 as N2O4?

Express your answer using four significant figures.

Part D

Rationalize the results from parts B and C by using Le Chatelier's principle (Section 15.7 in the textbook).

Expert Solution

queen_honey_blossom answered 2 years ago

N2O4 (g) ⇌ 2NO2(g). KP = 0.10 at some Temperature. If 0.40 atm of N2O4 is...

N2O4 (g) ⇌ 2NO2(g). KP = 0.10 at some Temperature. If 0.40 atm of N2O4 is placed in an evacuated flask, what are the pressures at equilibrium?

The half-life for the first-order decomposition of N2O4 is 1.3×10?5s. N2O4(g)?2NO2(g) Part A If N2O4 is...

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The degree of dissociation, α, for the following reaction: N2O4(g) <--> 2NO2(g) is 0.655 at 298...

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At 100∘C, Kc = 4.72 for the reaction 2NO2(g)⇌N2O4(g). An empty 10.0 L flask is filled...

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The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If...

The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If a reaction vessel at that temperature initially contains 0.030M NO2 and 0.030M N2O4, what are the concentrations of the two gases at equilibrium? First, the reaction quotient (Q) [page 645 of textbook] must be calculated, and then use the I.C.E table [page 648-650 of the textbook] to determine the equilibrium concentrations.

For the following reaction, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) If a reaction vessel initially...

For the following reaction, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) If a reaction vessel initially contains an N2O4 concentration of 5.50×10−2 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K? [N2O4], [NO2] = ____ M

At –80°C, K for the reaction N2O4(g) 2NO2(g) is 4.66 × 10–8. We introduce 0.049 mole...

At –80°C, K for the reaction N2O4(g) 2NO2(g) is 4.66 × 10–8. We introduce 0.049 mole of N2O4 into a 1.0-L vessel at –80°C and let equilibrium be established. The total pressure in the system at equilibrium will be: (0.78 atm)

For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a...

For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a reaction vessel initially contains an N2O4 concentration of 5.50×10−2 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K? [N2O4], [NO2] =

Consider the reaction N2O4 (g) ? 2 NO2 (g). At equilibrium, a 2.00-L reaction vessel contains...

Consider the reaction N2O4 (g) ? 2 NO2 (g). At equilibrium, a 2.00-L reaction vessel contains NO2 at a pressure of 0.269 atm and N2O4 at a pressure of 0.500 atm. The reaction vessel is then compressed to 1.00 L. What will be the pressures of NO2 and N2O4 once equilibrium is re-established?

Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium...

Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium partial pressures of NO2 and N2O4 are 1.337 atm and 0.657 atm, respectively.

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