Question

How many grams of aluminum are required to react with 35 mL of 2.0 M hydrochloric acid, HCl?__ HCl + __ Al --> __ AlCl3 + __ H2

Answer 1

0.6258 g

Step-by-step explanation:

To determine the number grams of aluminum in the above reaction;

• determine the number of moles of HCl
• determine the mole ratio,
• use the mole ratio to calculate the number of moles of aluminum.
• use RFM of Aluminum to determine the grams required.

Moles of HCl

35 mL of 2.0 M HCl

2 moles of HCl is contained in 1000 mL

x moles of HCl is contained in 35 mL

`x \: mol \: = \: (2 \: * \: 35)/(1000) \\ = 0.07 \: moles \:`

We have 0.07 moles of HCl.

Mole ratio

• Balanced equation

6HCl(aq) + 2Al(s) --> 2AlCl3(aq) + 3H2(g)

Hence mole ratio = 6 : 2 (HCl : Al

• but moles of HCl is 0.07, therefore the moles of Al;

`= (2)/(6) * 0.07 \\ \: = 0.0233333 \: moles`

Therefore we have 0.0233333 moles of aluminum.

Grams of Aluminum

We use the formula;

`grams \: = moles \: * \: rfm`

The RFM (Relative formula mass) of aluminum is 26.982g/mol.

Substitute values into the formula;

`= 0.0233333 \: moles \: * \: 26.982 \: (g)/(mol) \\ = 0.625799 \: grams`

The number of grams of aluminum required to react with HCl is 0.6258 g.