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18 Dec 2019

Suppose that a system initially contains 0.300 moles of N2O4 (g) and 0.500 moles of NO2 (g), and the equilibrium N2O4 (g) ⇋ 2NO2 (g) is attained at 25oC and 2.00 atm. Find the equilibrium composition and the standard free energy of the reaction.

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Related questions

Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ?C in a vessel that contains an initial N2O4 concentration of 0.0399M . The equilibrium constant Kc for the reaction N2O4(g)?2NO2(g) is 4.64

Consider the following reaction:

N2O4(g)⇌2NO2(g),Kc=0.36 at 100∘C

The reaction mixture initially contains only the reactant, [N2O4]=0.0218M , and no NO2.

Part A

Find the equilibrium concentration of N2O4.

Express the concentration to three decimal places and include the appropriate units.

Part B

Find the equilibrium concentration of NO2.

Express the concentration to three decimal places and include the appropriate units.

Dinitrogen tetroxide decomposes to nitrogen dioxide N2O4 (g)--> 2NO2 (g). Delta H =55.3kJ. At 298K a reaction vessel contains 0.100 atm of N2O4. When equilibrium is reached 58% of the N2O4 has decomppsed to NO2 What percentage of N2O4 decomposes at 380 K ? Assume that the initial pressure of N2O4 is the same (0.100 atm).

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