is formed is 0.050 M/s
is consumed is 0.0250 M/s.
![-\frac{1}{2}\frac{d[NO]}{dt}=-\frac{d[O_2]}{dt}=\frac{1}{2}\frac{d[NO_2]}{dt}](/tpl/images/0524/2208/cb5a7.png)
![\frac{d[NO]}{dt}=-0.050\ M/s](/tpl/images/0524/2208/0265a.png)
(Negative sign shows consumption)![-\frac{1}{2}\frac{d[NO]}{dt}=\frac{1}{2}\frac{d[NO_2]}{dt}](/tpl/images/0524/2208/0085e.png)
![-\frac{d[NO]}{dt}=\frac{d[NO_2]}{dt}](/tpl/images/0524/2208/49698.png)
![-(-0.050\ M/s)=\frac{d[NO_2]}{dt}](/tpl/images/0524/2208/98254.png)
![\frac{d[NO_2]}{dt}=0.050\ M/s](/tpl/images/0524/2208/27395.png)
![-\frac{1}{2}\frac{d[NO]}{dt}=-\frac{d[O_2]}{dt}](/tpl/images/0524/2208/fa609.png)
![-\frac{1}{2}\times -0.050\ M/s=-\frac{d[O_2]}{dt}](/tpl/images/0524/2208/649b1.png)
![\frac{d[O_2]}{dt}=0.0250\ M/s](/tpl/images/0524/2208/bc002.png)
Consider the reaction 2 NO + O2 → 2 NO2
Suppose that at a particular moment during the reactio...
Chemistry, 26.02.2020 01:46 231cornelius
Consider the reaction 2 NO + O2 → 2 NO2
Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.050 M/s.
(a) At what rate is NO2 being formed?
(b) At what rate is molecular oxygen reacting?
Answers: 1
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