What mass of oxygen is needed to react with 4.5g of ethane $C_{2} H_{8}$ $C_2H_8$ ?

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What mass of oxygen is needed to react with 4.5g of ethane $C_{2} H_{8}$ $C_2H_8$ ?

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Answer 1 · 2016-10-09T18:22:45

We need approx. $17 \cdot g$ $17*g$ of dioxygen.

Explanation:

A balanced chemical equation is required:

$H_{3} C - C H_{3} + \frac{7}{2} O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (g)$ $H_3C-CH_3 + 7/2O_2(g) rarr 2CO_2(g) +3H_2O(g)$

And thus each equiv ethane requires $\frac{7}{2}$ $7/2$ equiv of dioxygen.

$Moles of ethane$ $"Moles of ethane"$ $=$ $=$ $\frac{4.5 \cdot g}{30.07 \cdot g \cdot m o l^{- 1}}$ $(4.5*g)/(30.07*g*mol^-1)$ $=$ $=$ $0.15 \cdot m o l$ $0.15*mol$

And thus we need:

$\frac{7}{2} \times 0.15 \cdot m o l \times 32.00 \cdot g \cdot m o l^{- 1} dioxygen gas$ $7/2xx0.15*molxx32.00*g*mol^-1" dioxygen gas"$ $=$ $=$ $? ? g$ $??g$

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What mass of oxygen is needed to react with 4.5g of ethane $C_{2} H_{8}$ $C_2H_8$ ?

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What mass of oxygen is needed to react with 4.5g of ethane $C_{2} H_{8}$ $C_2H_8$ ?