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the total pressure of n2o4
92.01 grams of N2O4 (g) is placed in a container and allowed to dissociate.
N2O4 (g) --> 2NO2 (g) The mixture of N2O4 and NO2
2 answers
asked by
Neha
953 views
Dinitrogen tetroxide decomposes according to N2O4 (g) = 2NO2 (g)
In a certain experiment, N2O4(g) at an initial pressure of 0.554
1 answer
asked by
Angel
1,479 views
the total pressure of n2o4 and no2 IS 1.38 atm. if kp is 6.75(25 C) calculate partial pressure of NO2 in the mixture. 2NO2<--->
5 answers
asked by
anon
1,193 views
1-Dinitrogen tetroxide (N2O4) dissociates according to the equation:
N2O4 ⇌ 2NO2 An equilibrium reaction mixture at 25 ºC was
3 answers
asked by
John
1,837 views
At 25∘C, 0.11 mol of N2O4 reacts to form 0.10 mol of N2O4 and 0.02 mol of NO2. At 90∘C, 0.11 mol of N2O4 forms 0.050 mol of
2 answers
asked by
Person
536 views
How does increasing the pressure on this system affect the amount of N2O4 formed?
The amount of N2O4 remains the same. The amount
1 answer
50 views
Consider the following reaction.
2NO2(g)⇌N2O4(g) When the system is at equilibrium, it contains NO2 at a pressure of 0.724 atm
1 answer
asked by
BBaa
2,074 views
The half-life for the first-order decomposition of is 1.3*10^-5.
N2O4--> 2NO2 If N2O4 is introduced into an evacuated flask at a
2 answers
asked by
Anonymous
2,782 views
Consider the following equilibrium:
N2O4 <=> 2NO2 You may assume that delta H and delta S do not vary with temperature. At what
0 answers
asked by
John
1,250 views
Dinitrogen tetroxide decomposes to nitrogen dioxide:
N2O4 (g) ---> 2NO2 (g) Delta H rxn: 55.3 kJ At 298 K a reaction vessel
1 answer
asked by
Tyler
2,264 views