Colourless N2O4 decomposes to form brown NO2, in a first order reaction. The following values were...
Colourless N2O4 decomposes to form brown NO2, in a
first order reaction. The following values
were determined for k.
N2O4(g) ⎯→ 2NO2(g)
k = 4.5 x 10
3 s
-1 at 274 K
k = 1.00 x 104 s
-1 at 283 K
By making use of this information, calculate the value of Ea.
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Colourless N2O4 decomposes to form brown NO2, in a
first order reaction. The following values
were...
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When heated, colorless dinitrogen tetraoxide, N2O4(g), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204 (g) + 2 NO2 (g) Suppose that 2.00 mol of N204(g) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K, for this reaction at 407 K. 3.80 2.00 0.500 0.263 0.525
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When heated, colorless dinitrogen tetraoxide, N2O4(g), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204 (g) + 2 NO2 (g) Suppose that 2.00 mol of N204(g) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K, for this reaction at 407 K. 3.80 2.00 0.500 0.263 0.525
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