How many moles of hydrogen would be obtained if 2.7g of aluminium reacts with excess hydrochloric acid?

2Al + 6HCl = 2AlCl3 + 3H2

So, how many moles in 2.7g of Al?
You get 3/2 times that many moles of H2

To determine the number of moles of hydrogen produced when 2.7g of aluminum reacts with excess hydrochloric acid, we need to follow these steps:

Step 1: Determine the molar mass of aluminum (Al).
The molar mass of Al is 26.98 g/mol.

Step 2: Convert the given mass of aluminum (2.7g) to moles.
Using the formula: Moles = Mass / Molar mass
Moles of Al = 2.7g / 26.98 g/mol = 0.1 mol

Step 3: Determine the balanced chemical equation for the reaction.
For the reaction between aluminum and hydrochloric acid (HCl):
2 Al + 6 HCl → 2 AlCl3 + 3 H2

Step 4: Calculate the molar ratio.
From the balanced equation, we see that:
2 moles of aluminum react to produce 3 moles of hydrogen.

Step 5: Calculate the moles of hydrogen produced.
Using the ratio obtained in Step 4:
Moles of H2 = Moles of Al / ratio
Moles of H2 = 0.1 mol / (2/3) = 0.15 mol

Therefore, 0.15 moles of hydrogen would be obtained when 2.7g of aluminum reacts with excess hydrochloric acid.

To find out how many moles of hydrogen would be obtained in this reaction, we need to use the balanced chemical equation for the reaction between aluminium and hydrochloric acid.

The balanced chemical equation for the reaction is:

2Al + 6HCl -> 2AlCl3 + 3H2

From the equation, we can see that 2 moles of aluminium react with 6 moles of hydrochloric acid to produce 3 moles of hydrogen.

Next, we need to determine the number of moles of 2.7g of aluminium. To do this, we'll use the molar mass of aluminium.

The molar mass of aluminium (Al) is 26.98 g/mol.

Using the equation:

moles = mass / molar mass

we can find the moles of aluminium:

moles of aluminium = 2.7g / 26.98 g/mol

moles of aluminium = 0.1 mol

Since there is an excess of hydrochloric acid in the reaction, we can assume that all the aluminium reacts completely.

From the balanced equation, we know that 2 moles of aluminium react to produce 3 moles of hydrogen. Therefore, the moles of hydrogen produced would be:

moles of hydrogen = (moles of aluminium) * (3 moles of hydrogen / 2 moles of aluminium)

moles of hydrogen = 0.1 mol * (3/2)

moles of hydrogen = 0.15 mol

So, 0.15 moles of hydrogen would be obtained when 2.7g of aluminium reacts with excess hydrochloric acid.