Question

5.6
The drain cleaner, Drainex contains small bits of aluminum which react with caustic soda to produce dihydrogen. What volume of dihydrogen at 20 °C and one bar will be released when 0.15g of aluminum reacts?
pls answer with step by step explanation ​

Answer 1

Answer:

$\huge\color{YELLOW}\mathbb{ANSWER}$

Explanation:

The reaction can be written as :-

$2Al_{s} + 2NaOH_{(aq)} + 2H_{2}O_{l}⟶</p><p>2NaAlO{2(aq)}+_{3}H_{2(g)}$

Here, 2 moles of Al gives 3 moles of $H_{2}$ gas.

Moles of aluminium$=  \frac{ 0.15g}{27}=5.56× {10}^{−3}moles$

∴Moles of $H_{2}$ produced$=  \frac{3}{2} ×5.56×{10}^{−3}=8.33×{10}^{−3} moles$

$∴Volume\:of\:H_{2} = \frac{nRT}{ P}</p><p></p><p>= \frac{ 8.33×10−3×0.0831×293}{1} \\ =0.203 litres \\ </p><p>∴ Volume\:of\:di\:hydrogen\:released\:is 0.203\:litres$

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