Gaseous azomethane, CH3N=NCH3 , decomposes in a first-order reaction when heated: CH3N=NCH3(g) ---->N2 (g) + C2H6...
Gaseous azomethane, CH3N=NCH3 , decomposes in a first-order reaction when heated:
CH3N=NCH3(g) ---->N2 (g) + C2H6 (g)
The rate constant for this reaction at 600 K is 0.0216 .
a. If the initial quantity of azomethane in the flask is 4.64 g, how much remains after 0.0510 hour?
b. how many grams of N2?
Homework Answers
You are missing the unit of rate constant i.e
K = 0.0216 hour^-1 or min^-1 or sec^-1
I'm assuming it to be hour to calculate it .
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Gaseous azomethane, CH3N=NCH3 , decomposes
in a first-order reaction when heated:
CH3N=NCH3(g) ---->N2 (g) +
C2H6...
Gaseous azomethane, CH3N=NCH3, decomposes in a first-order reaction when heated: CH3N=NCH3(g) → N2(g) + C2H6(g) (A)...
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First-Order Reactions (35) Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g) — N2(g) + C2H6(g) The following data are obtained in an experiment: Time (h) [(CH3)2N2] 1.00 0.905 2.00 0.741 3.00 0.607 4.00 0.497 (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time in hours) that it takes decrease the concentration to 0.100 M. (d) Calculate...
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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at 327 oC is k = 3.60e-04 s-1. Suppose we
start with 0.0505 mol of CH3N2CH3
in a volume of 3.7 L. How many moles of
CH3N2CH3 will remain after
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a) 0.0224 moles will remain.
b) 0.000684 moles will remain.
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