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Calorimetry

In the follow...

Question

In the following reaction $2 H_{2} O_{2} (a q) \to 2 H_{2} O (ℓ) + O_{2} (g)$ rate of formation of $O_{2} is 36 g {min}^{- 1},$
(a) What is the rate of formation of $H_{2} O$
(b) What is the rate of disappearance of $H_{2} O$ .

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Solution

$2 H_{2} O_{2}$ (aq) $\to$ $2 H_{2} O (l) + O_{2}$ $(g)$
Now, Rate= $- \frac{1}{2}$ $\frac{d}{d t}$ $H_{2}$ $O_{2}$
= $- \frac{1}{2}$ $\frac{d}{d t}$ $H_{2}$ $O$
= $\frac{d}{d t}$ $[O_{2}]$
Rate of formation of $O_{2}$ = $\frac{d}{d t}$ $O_{2}$ =36 g ${m i n}^{- 1}$
Rate of formation of $H_{2}$ O= $\frac{d}{d t}$ [ $H_{2}$ O]
=2 $\times$ $\frac{d}{d t}$ $[O_{2}]$
=2 $\times 36 g {m i n}^{- 1}$
Rate of formation of $H_{2}$ O= $72 g {m i n}^{- 1}$
Rate of disappearance of $H_{2}$ O= $- \frac{d}{d t}$ [ $H_{2}$ $O_{2}$ ]
=2 $\times$ $\frac{d}{d t}$ $[O_{2}]$
=2 $\times 36 g {m i n}^{- 1}$
Rate of formation of $H_{2}$ O= $72 g {m i n}^{- 1}$

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