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Consider the following reaction:
2Al (s) + 6HCl (aq) → 2AlCl3 (aq) + 3H2 (g).
A 0.080 mole piece of aluminum reacted completely in 20 s.
The rate of formation of hydrogen gas is:

Sagot :

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The rate of formation of hydrogen gas is:

  • [tex]0.006mol/s[/tex]

Chemical equation

2Al (s) + 6HCl (aq) → 2AlCl3 (aq) + 3H2 (g).

According to the reaction,

2mol Al can produce 3mol [tex]H_2[/tex]

0.08mol Al = [tex]\frac{3*0.08}{2}mol H_2[/tex]

[tex]= 0.12mol H_2[/tex]

so we can say,

in 20s, 0.12mol H_2 will be produced

Hydrogen Formation

The rate of formation of [tex]H_2[/tex] = [tex]\frac{mol of H_2 formed}{time taken to form}[/tex]

[tex]= \frac{0.12}{20}\\\\= 0.006mol/s[/tex]

For more information on formation of hydrogen, visit

https://brainly.com/question/9791360?referrer=searchResults

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