Consider this reaction: →NH4OHaq+NH3aqH2Oaq At a certain temperature it obeys this rate law.rate =·26.0M−1s−1NH4OH2 Suppose a vessel contains NH4OH at a concentration of 1.28M. Calculate the concentration of NH4OH in the vessel 0.270 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits. =___M
Consider this reaction:
At a certain temperature it obeys this rate law.rate
Suppose a vessel contains NH4OH at a concentration of 1.28M. Calculate the concentration of NH4OH in the vessel 0.270 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits.
=___M
Given: Decomposition of ammonium hydroxide which is a second order Reaction.
Rate constant= 26.0 M-1s-1
Concentration of NH4OH= 1.28 M
To find:Concentration of NH4OH left ater 0.270 seconds.
Solution: Chemical kinetics is one of the most important branch of Physical chemistry.
Chemical kinetics deals with the study of the rate of reaction. But only the rated of moderate reactions can be determined.
It is a second order Reaction as seen from the rate law or the units of rate constant.
For second order Reaction we can use the formula as shown below:
K=1/t [(1/at)-(1/a0)]
Where K is rate constant
t is time
at is final concentration
a0 is initial concentration.
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