What is the minimum amount of 6.0 M H2SO4 necessary to produce 19.0 g of H2(g) according to the reaction?
2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)
From given reaction equation, moles acid consumed = moles H2 produced = 19g/2g/mole = 9.5 moles acid = Molarity x Volume(L) = 6M x Vol(L) => 1.583 Liters of the Acid Solution
Well, let's analyze this equation, shall we? According to the equation, we need 3 moles of H2SO4 to produce 3 moles of H2. So to find out the minimum amount of H2SO4 required, we need to first determine the number of moles of H2.
Given that the molar mass of H2 is approximately 2 g/mol, we can calculate the number of moles of H2:
19.0 g H2 / 2 g/mol = 9.5 moles of H2
Since the stoichiometric ratio between H2SO4 and H2 is 3:3 (or simply 1:1), we need an equal amount of moles of H2SO4. Therefore, we need a minimum of 9.5 moles of 6.0 M H2SO4.
Now, to find the amount of solution needed, we can use the formula:
Molarity (M) = Moles / Volume (L)
Rearranging the formula to solve for volume:
Volume (L) = Moles / Molarity
Volume (L) = 9.5 moles / 6.0 M = 1.58 L
So, the minimum amount of 6.0 M H2SO4 necessary would be approximately 1.58 liters. But of course, don't forget to bring your own flask and a clown nose for the experiment! 🤡
To determine the minimum amount of 6.0 M H2SO4 necessary to produce 19.0 g of H2(g) according to the given reaction, we need to use stoichiometry.
1. Start by balancing the chemical equation if necessary:
2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
2. Convert the given mass of H2(g) to moles:
Using the molar mass of H2, which is 2.02 g/mol, we can calculate the number of moles:
19.0 g H2 × (1 mol H2 / 2.02 g H2) = 9.41 mol H2
3. Use the stoichiometry of the balanced equation to find the moles of H2SO4 needed:
From the balanced equation, we can see that for every 3 moles of H2SO4, we produce 3 moles of H2. Therefore, the ratio is 3 moles of H2SO4 per 3 moles of H2, or 1 mole of H2SO4 per 1 mole of H2.
So, the number of moles of H2SO4 needed is also 9.41 mol.
4. Calculate the volume of 6.0 M H2SO4 needed based on its concentration:
The concentration of 6.0 M H2SO4 means that there are 6.0 moles of H2SO4 in 1 liter (or 1000 mL) of solution.
Since we need 9.41 moles of H2SO4, we can use the following conversion:
(9.41 mol H2SO4) × (1 L H2SO4 / 6.0 mol H2SO4) = 1.57 L
Therefore, the minimum amount of 6.0 M H2SO4 necessary to produce 19.0 g of H2(g) is 1.57 liters.
To determine the minimum amount of 6.0 M H2SO4 required to produce 19.0 g of H2(g), we need to calculate the limiting reactant in the given reaction and then determine the stoichiometry between the limiting reactant and the desired product (H2 gas).
Here's how to approach the problem:
Step 1: Calculate the molar mass of H2(g)
The molar mass of H2 is 2.02 g/mol since hydrogen gas (H2) consists of two hydrogen atoms.
Step 2: Determine the number of moles of H2(g)
To find the number of moles of H2, divide the given mass (19.0 g) by the molar mass of H2:
Number of moles = Mass / Molar mass
Number of moles of H2 = 19.0 g / 2.02 g/mol
Step 3: Write a balanced equation and determine the mole ratio
The balanced equation shows that 3 moles of H2SO4 react with 3 moles of H2 to form 3 moles of H2. Therefore, the mole ratio of H2SO4 to H2 is 1:1.
Step 4: Calculate the moles of H2SO4 required
Since the mole ratio of H2SO4 to H2 is 1:1, the amount of moles of H2SO4 needed is the same as the number of moles of H2.
Step 5: Calculate the volume of 6.0 M H2SO4 required
Finally, use the molarity and the moles of H2SO4 to calculate the volume of H2SO4 required. The molarity is given as 6.0 M, which means there are 6.0 moles of H2SO4 per liter of solution. Divide the calculated moles of H2SO4 by the molarity to determine the volume in liters.
To summarize,
1. Calculate the molar mass of H2(g).
2. Determine the number of moles of H2(g).
3. Write and balance the chemical equation to determine the stoichiometric ratio.
4. Determine the moles of H2SO4 required.
5. Calculate the volume of 6.0 M H2SO4 needed.
mols H2 gas = grams/molar mass = 19/2.0 = 9.5
mols H2SO4 needed = 9.5 since 1 mol H2SO4 = 1 mol H2 in the balanced equation.
M = mols/L or 6.0 = 9.5/L and L = 9.5/6.0 = 1.583 which I would round to 1.58 L.