The decomposition of NH3 on platinum surface is zero order reaction. If rate constant (k) is 4 × 10^–3 Ms–1, how long will it take to reduce the initial concentration of NH3 from 0.1 M to 0.064 M.
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Answer:
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Answer:
it will take 9.0 × 10^3 seconds, or 2.5 hours (rounded to the nearest half hour), to reduce the initial concentration of NH3 from 0.1 M to 0.064 M.
Explanation:
For a zero-order reaction, the rate equation is given by:
Rate = k
where k is the rate constant.
The rate of the reaction is independent of the concentration of the reactant(s). This means that the rate of the reaction remains constant throughout the reaction, and is equal to the rate constant.
The integrated rate equation for a zero-order reaction is given by:
[A]t = [A]0 - kt
where [A]t is the concentration of the reactant at time t, [A]0 is the initial concentration of the reactant, k is the rate constant, and t is the time.
In this case, we are given that the rate constant (k) is 4 × 10^–3 Ms^–1, the initial concentration ([A]0) is 0.1 M, and we want to know the time it takes to reduce the concentration to 0.064 M ([A]t).
Substituting these values into the integrated rate equation, we get:
0.064 M = 0.1 M - (4 × 10^–3 Ms^–1) t
Solving for t, we get:
t = (0.1 M - 0.064 M) / (4 × 10^–3 Ms^–1)
t = 9.0 × 10^3 s
Therefore, it will take 9.0 × 10^3 seconds, or 2.5 hours (rounded to the nearest half hour), to reduce the initial concentration of NH3 from 0.1 M to 0.064 M.
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