What volume of dioxygen gas would be generated by complete decomposition of a $10 \cdot g$ $10g$ mass of $K C l O_{3}$ $KClO_3$ , under a pressure of $750 \cdot m m \cdot H g$ $750mm*Hg$ ?

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What volume of dioxygen gas would be generated by complete decomposition of a $10 \cdot g$ $10g$ mass of $K C l O_{3}$ $KClO_3$ , under a pressure of $750 \cdot m m \cdot H g$ $750mm*Hg$ ?

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Answer 1 · 2017-09-03T06:36:47

Well, we need a stoichiometric equation......and I get under $2 \cdot L$ $2*L$ .

Explanation:

$K C l O_{3} M n O_{2} - -- \to \frac{3}{2} O_{2} (g) + K C l$ $KClO_3stackrel(MnO_2)rarr3/2O_2(g) + KCl$

Some $M n (I V)$ $Mn(IV)$ salt is usually added to catalyze the reaction.

$Moles of potassium chlorate = \frac{10 \cdot g}{122.55 \cdot g \cdot m o l^{- 1}}$ $"Moles of potassium chlorate"=(10*g)/(122.55*g*mol^-1)$

$= 0.0816 \cdot m o l$ $=0.0816*mol$

And thus we gets $\frac{3}{2} \times 0.0816 \cdot m o l = 0.122 \cdot m o l$ $3/2xx0.0816*mol=0.122*mol$ $dioxygen gas$ $"dioxygen gas"$ .

And then we simply solve the Ideal Gas equation.....

$V = \frac{n R T}{P} = \frac{0.0816 \cdot m o l \times 0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 291 \cdot K}{\frac{750 \cdot m m \cdot H g}{760 \cdot m m \cdot H g \cdot a t m^{- 1}}}$ $V=(nRT)/P=(0.0816*molxx0.0821*(L*atm)/(K*mol)xx291*K)/((750*mm*Hg)/(760*mm*Hg*atm^-1))$

$= ? ? \cdot L$ $=??*L$

Note the pressure measurement. A mercury column is a VERY convenient means to measure gas pressure in that we know that $1 \cdot a t m$ $1*atm$ will support a column of mercury that is $760 \cdot m m$ $760*mm$ high. These days mercury has all but disappeared from laboratories because of perceived safety concerns. (I keep my manometers under lock and key, away from nosy safety inspectors).

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What volume of dioxygen gas would be generated by complete decomposition of a $10 \cdot g$ $10g$ mass of $K C l O_{3}$ $KClO_3$ , under a pressure of $750 \cdot m m \cdot H g$ $750mm*Hg$ ?

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What volume of dioxygen gas would be generated by complete decomposition of a 10⋅g10*g mass of KClO3KClO_3, under a pressure of 750⋅mm⋅Hg750*mm*Hg?

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Explanation:

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What volume of dioxygen gas would be generated by complete decomposition of a $10 \cdot g$ $10g$ mass of $K C l O_{3}$ $KClO_3$ , under a pressure of $750 \cdot m m \cdot H g$ $750mm*Hg$ ?