According to the reaction 2Al+3H2SO4→3H2+Al2(SO4)3, the total number of moles of H2SO4 needed to react completely with 5.0 mol of AL is
1. 2.5 mol
2. 5.0 mol
3. 7.5 mol
4. 9.0 mol
7.5
The "coefficient factor" will convert any thing to anything.
5.0 mol Al x (3 mols H2SO4/2 mols Al) = 5.0 x 3/2 = ?
Well, what you have here is a chemical reaction and you're trying to determine the amount of H2SO4 needed to react with 5.0 moles of Al. Since the balanced equation tells us that the ratio of Al to H2SO4 is 2:3, we know that for every 2 moles of Al, we need 3 moles of H2SO4. So if you have 5.0 moles of Al, you can just set up a simple proportion:
(2 moles Al / 3 moles H2SO4) = (5.0 moles Al / x moles H2SO4)
Solving for x, we find that x = (5.0 moles Al) * (3 moles H2SO4 / 2 moles Al) = 7.5 moles H2SO4.
So the correct answer is 3. 7.5 mol.
To determine the total number of moles of H2SO4 needed to react completely with 5.0 mol of Al, we need to use the balanced chemical equation and the stoichiometric ratios.
According to the reaction equation: 2Al + 3H2SO4 → 3H2 + Al2(SO4)3
The stoichiometric ratio between Al and H2SO4 is 2:3. This means that for every 2 moles of Al, we need 3 moles of H2SO4.
In this case, we have 5.0 mol of Al. To find the number of moles of H2SO4 needed, we can set up a ratio using the stoichiometric ratio:
(5.0 mol Al) x (3 mol H2SO4 / 2 mol Al) = 7.5 mol H2SO4
Therefore, the total number of moles of H2SO4 needed to react completely with 5.0 mol of Al is 7.5 mol.
So the correct answer is option 3: 7.5 mol.
i too am hopeless when asked this question
9.0
67.73 g
i dont now the anzer!