chmereaustin1

21.05.2020 • 

Chemistry

Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism:
step elementary reaction rate constant
1 NO2 (g) → NO (g) + O (g) k1
2 O (g) + NO2 (g) → O2 (g) + NO (g) k2
Suppose also k1>>k2. That is, the first step is much faster than the second.
(a) Write the balanced chemical equation for the overall chemical reaction.
(b) Write the experimentally-observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates.
(c) Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k.2 for the reverse of the two elementary reactions in the mechanism.

Ответ:

carlo123

25.06.2022

Chemistry

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The concentration (in mM units) of vitamin C in the juice is 0.64mM.

Explanation:

Let us calculate -:

Concentration of sample =>

                               = 29.4 mmol => 29.4mmol/50ml

                               = 0.588mM

plug in formula => or

= [2.02 micro-Amber/3.79micro-Amber]

plug in and simplify

1.81x = 1.17

x = 0.64mM

Hence , the answer is 0.64mM.

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