Integrated rate law homework equations Gen Chem II

[DMB]

Homework Statement

Integrated rate law calculations

Relevant Equations

The decomposition of ammonia on a platinum surface at 856 °C

NH31/2 N2 + 3/2 H2

is zero order in NH3 with a rate constant of 1.50×10-6M s-1.
If the initial concentration of NH3 is 5.28×10-3 M, the concentration of NH3 will be ___
M after 2.54×103seconds have passed.
The decomposition of nitrosyl bromide at 10 °C

NOBrNO + ½ Br2

is second order in NOBr.

In one experiment, when the initial concentration of NOBr was 0.341 M, the concentration of NOBr dropped to 7.81×10-2 M after 9.06seconds had passed.

Based on these data, the rate constant for the reaction is ___
M-1 s-1.
The gas phase decomposition of nitrogen dioxide at 383 °C

NO2(g)NO(g) + ½ O2(g)

is second order in NO2 with a rate constant of 0.540M-1 s-1.

If the initial concentration of NO2 is 0.131 M, the concentration of NO2 will be 3.28×10-2 M after
___ seconds have passed.

No idea how to solve

 

[chemisttree]

Homework Statement:: The decomposition of ammonia on a platinum surface at 856 °C

NH₃ --> 1/2 N₂ + 3/2 H₂

is zero order in NH₃ with a rate constant of 1.50×10^-6M s-1.
If the initial concentration of NH₃ is 5.28×10^-3 M, the concentration of NH₃ will be ___M after 2.54×10³ seconds have passed.

No idea how to solve

I’ve cleaned up your “stuff” a little for clarity. You actually asked three questions so let’s start with the first one.

What does it mean to be “zero order” with respect to NH₃?

 

[chemisttree]

You need only to put in the mildest of efforts if you want help in the HW forum...

 

[epenguin]

First post by student who has apparently not realized nature and ethos of this site and of Homework Help. He has not only put no effort towards answering but also none into asking the question. None of the chemical reactions are written out properly. Should check site Homework Help instructions - it says "no idea" is the very thing not to say.

These are straight out-of-the-textbook questions, how to do are in every textbook of chemical kinetics or University-level general physical chemistry.