Chemistry, 26.02.2020 17:00, manillasoccer
Consider the following balanced chemical equation. 4 KO 2 + 2 H 2 O ⟶ 4 KOH + 3 O 2 How is the rate of appearance of O 2 , Δ [ O 2 ] Δ t , related to the rate of disappearance of KO 2 ?
Answers: 3
related to the rate of disappearance of 
is,![\frac{d[O_2]}{dt}=-\frac{3}{4}\frac{d[KO_2]}{dt}](/tpl/images/0524/9521/55d25.png)
![\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}](/tpl/images/0524/9521/2d8eb.png)
![\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}](/tpl/images/0524/9521/1e77e.png)
![\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}](/tpl/images/0524/9521/cee4b.png)
![\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}](/tpl/images/0524/9521/7ef32.png)
![Rate=-\frac{1}{a}\frac{d[A]}{dt}=-\frac{1}{b}\frac{d[B]}{dt}=+\frac{1}{c}\frac{d[C]}{dt}=+\frac{1}{d}\frac{d[D]}{dt}](/tpl/images/0524/9521/d4b94.png)
![\text{Rate of disappearance of }KO_2=-\frac{1}{4}\frac{d[KO_2]}{dt}](/tpl/images/0524/9521/4cd78.png)
![\text{Rate of disappearance of }H_2O=-\frac{1}{2}\frac{d[H_2O]}{dt}](/tpl/images/0524/9521/6a91b.png)
![\text{Rate of formation of }KOH=+\frac{1}{4}\frac{d[KOH]}{dt}](/tpl/images/0524/9521/9b206.png)
![\text{Rate of formation of }O_2=+\frac{1}{3}\frac{d[O_2]}{dt}](/tpl/images/0524/9521/e5480.png)
![\text{Rate of reaction}=-\frac{1}{4}\frac{d[KO_2]}{dt}=-\frac{1}{2}\frac{d[H_2O]}{dt}=+\frac{1}{4}\frac{d[KOH]}{dt}=+\frac{1}{3}\frac{d[O_2]}{dt}](/tpl/images/0524/9521/7ae32.png)
![-\frac{1}{4}\frac{d[KO_2]}{dt}=+\frac{1}{3}\frac{d[O_2]}{dt}](/tpl/images/0524/9521/ab2f5.png)
![+\frac{1}{3}\frac{d[O_2]}{dt}=-\frac{1}{4}\frac{d[KO_2]}{dt}](/tpl/images/0524/9521/4e479.png)
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Consider the following balanced chemical equation. 4 KO 2 + 2 H 2 O ⟶ 4 KOH + 3 O 2 How is the rate...
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