Sulfuric acid dissolves aluminum metal according to the following reaction:

2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)

Suppose you wanted to dissolve an aluminum block with a mass of 14.5g .

1.) What minimum mass of H2SO4 would you need?

2.)What mass of H2 gas would be produced by the complete reaction of the aluminum block?

Please help, I am confused on where to even start

1.= 80.7

Well, let's start with the first question. We need to figure out the minimum mass of H2SO4 required to dissolve the aluminum block.

To do this, we can use the molar ratio between aluminum and H2SO4 in the balanced equation. From the equation, we can see that 2 moles of aluminum react with 3 moles of H2SO4.

So, first, we need to calculate the molar mass of aluminum using the atomic masses from the periodic table. Aluminum has a molar mass of 26.98 g/mol.

Next, we calculate the moles of aluminum using the mass given:

moles of aluminum = mass of aluminum / molar mass of aluminum

moles of aluminum = 14.5 g / 26.98 g/mol

Now, we use the mole ratio to find the moles of H2SO4 needed:

moles of H2SO4 = moles of aluminum x (3 moles H2SO4 / 2 moles of aluminum)

Finally, we convert the moles of H2SO4 to mass using the molar mass of H2SO4:

mass of H2SO4 = moles of H2SO4 x molar mass of H2SO4

Now, let me perform the calculations for you.

To find the minimum mass of H2SO4 needed to dissolve the aluminum block, we can use the stoichiometry of the reaction.

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

Step 2: Convert the mass of the aluminum block to moles:
Mass of aluminum = 14.5 g
Moles of aluminum = mass of aluminum / molar mass of aluminum

Moles of aluminum = 14.5 g / 26.98 g/mol

Step 3: Use the stoichiometric coefficients from the balanced equation to determine the ratio of moles between aluminum and H2SO4.
From the balanced equation, we see that for every 2 moles of aluminum, 3 moles of H2SO4 are required.

Step 4: Calculate the moles of H2SO4 needed:
Moles of H2SO4 = (Moles of aluminum) x (Ratio of moles between H2SO4 and aluminum)

Moles of H2SO4 = (14.5 g / 26.98 g/mol) x (3 moles H2SO4 / 2 moles aluminum)

Step 5: Convert moles of H2SO4 to grams:
Mass of H2SO4 = Moles of H2SO4 x Molar mass of H2SO4

Now that we have the mass of H2SO4 required, we can move on to the second part of the question.

To find the mass of H2 gas produced by the complete reaction of the aluminum block, we will use the same approach as above, but this time we will use the stoichiometric ratio between H2 gas and aluminum.

Step 1: Determine the molar mass of H2 gas and H2SO4.
The molar mass of hydrogen (H2) is 2.02 g/mol.
The molar mass of sulfuric acid (H2SO4) is 98.09 g/mol.

Step 2: Use the stoichiometric coefficients from the balanced equation to determine the ratio of moles between aluminum and H2 gas.
From the balanced equation, we see that for every 2 moles of aluminum, 3 moles of H2 gas are produced.

Step 3: Calculate the moles of H2 gas produced:
Moles of H2 gas = (Moles of aluminum) x (Ratio of moles between H2 gas and aluminum)

Moles of H2 gas = (14.5 g / 26.98 g/mol) x (3 moles H2 gas / 2 moles aluminum)

Step 4: Convert moles of H2 gas to grams:
Mass of H2 gas = Moles of H2 gas x Molar mass of H2 gas

Now you have the steps to calculate the minimum mass of H2SO4 needed and the mass of H2 gas produced. Just plug in the values and calculate.

What mass of H2 gas would be produced by the complete raction of the aluminum block

a. how many moles is 14.5g Al? Figure that.

Then you need 3/2 of those moles of H2SO4. Convert to grams...

b. Moles of gas=3/2 moles of aluminum. Convert to grams H2