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The equilibrium system N2O4(g) 2NO2(g)

A 1.00 mol sample of N2O4 (g) is placed in a 10.0 L vessel and allowed to reach equilibrium accourding to the equationN2O4(g)
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2. asked by kevin
3. 3,673 views
Dinitrogen tetroxide decomposes to nitrogen dioxide:N2O4 (g) ---> 2NO2 (g) Delta H rxn: 55.3 kJ At 298 K a reaction vessel
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2. asked by Tyler
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The equilibrium system N2O4(g) 2NO2(g) was established in a 1.00-liter vessel. Upon analysis, the following information was
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2. asked by Chiara
3. 1,594 views
In the chemical reaction where N2O4(g) is converted to 2NO2(g), if 0.5 M N2O4 and 0.15 M NO2 are present in the vessel, is the
1. 3 answers
2. asked by Christine
3. 2,866 views
When heated, N2O4 dissociates as follows: N2O4 =2NO2A flask initially contians .560 M N2O4. at this temperature, Kc is 4.00.
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2. asked by Rob
3. 1,053 views
Dinitrogen tetroxide decomposes to nitrogen dioxide:N2O4(g)→2NO2(g)ΔHorxn=55.3kJ At 298 K, a reaction vessel initially
1. 1 answer
2. asked by Justiss
3. 4,796 views
In the chemical reaction where 0.1 M of N2O4 (g) is converted to 2NO2 (g), what are the concentration values of NO2 (g) in the
1. 6 answers
2. asked by Anonymous
3. 2,017 views
At 55C, the K for the reaction: 2NO2(g) <--> N2O4 is 1.15a) write the equilibrium expression b) calculate the concentration of
1. 5 answers
2. asked by Anonymous
3. 1,416 views
Dinitrogentetraoxide partially decomposes according to the following equilibrium:N2O4 (g) -> 2NO2 (g) <- A 1.00-L flask is
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2. asked by Jane
3. 4,203 views
i already posted this question, but im still confused on it.Dinitrogentetraoxide partially decomposes according to the following
1. 2 answers
2. asked by Jane
3. 2,955 views