Answer:
a) The average rate of decomposition of NOBr over the entire reaction is 3.4 x 10⁻⁴ M/s
b) The average rate of decomposition of NOBr between 2.00 and 4.00 seconds is 4 x 10⁻⁴ M/s
Explanation:
The average rate of decomposition of a reactant can be written as follows:
v = -1/a Δ[A] / Δt
Where
v: average rate of decomposition of A
a: stoichiometric coefficient of reactant A
Δ[A]: variation of the concentration of reactant A
(final concentration of A - initial concentration of A)
Δt: variation of time (final time - initial time)
a) The average rate of the decomposition of NOBr over the entire experiment can be calculated as follows, using this data:
Initial concentration of NOBr: 0.0100 M
Final concentration of NOBr: 0.0033 M
Initial time: 0.00 s
Final time: 10.00 s
Stoichiometric coefficient of NOBr: 2
Then:
v = -1/2 Δ[NOBr] / Δt
v = -1/2 (0.0033 M - 0.0100 M) / (10.00 s - 0.00 s) = 3.4 x 10⁻⁴ M/s
b) In the same way, the rate of decomposition can be calculated between the 2.00 and 4.00 seconds:
v = -1/2 (0.0055 M - 0.0071 M) / (4.00 s - 2.00 s) = 4 x 10⁻⁴ M/s
