What is the minimum amount of 5.0M H2So4 necessary to produce 24.1g of H2(g) according to the following reaction? 2Al(s) +3H2So4(aq) produces Al2(So4)3(aq) + 3H2(g)
I thought Bob Pursley gave you some hints to this problem. Here is a sample stoichiometry problem I've posted. Just follow the steps. M x L = moles. http://www.jiskha.com/science/chemistry/stoichiometry.html
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To determine the minimum amount of 5.0M H2SO4 necessary to produce 24.1g of H2(g), we need to convert the given mass of H2 to moles and then use the stoichiometry of the reaction to calculate the required moles of H2SO4.
Step 1: Calculate moles of H2
The molar mass of H2 is 2.02 g/mol.
Moles of H2(g) = mass of H2(g) / molar mass of H2(g)
Moles of H2(g) = 24.1g / 2.02g/mol
Moles of H2(g) ≈ 11.94 mol
Step 2: Use stoichiometry to find moles of H2SO4
According to the balanced chemical equation:
2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
The stoichiometric ratio between H2SO4 and H2 is 3:3, or 1:1.
Therefore, the moles of H2SO4 required will be approximately the same as the moles of H2(g), which is 11.94 mol.
Step 3: Calculate the volume of 5.0M H2SO4 needed
The molarity (M) of a solution is defined as moles of solute divided by liters of solution.
Moles of H2SO4 = Molarity × Volume (in liters)
11.94 mol = 5.0 M × Volume (in liters)
Solving for the volume:
Volume (in liters) = 11.94 mol / 5.0 M
Volume (in liters) ≈ 2.39 L
Therefore, the minimum amount of 5.0M H2SO4 necessary to produce 24.1g of H2(g) is approximately 2.39 liters.
To determine the minimum amount of 5.0M H2SO4 necessary to produce 24.1g of H2(g) according to the given reaction, we need to use stoichiometry.
Step 1: Calculate the molar mass of H2(g)
The molar mass of H2 is 2.016 g/mol.
Step 2: Convert the given mass of H2(g) to moles
The given mass is 24.1 g. We divide this by the molar mass of H2(g) to get the number of moles.
Moles of H2 = 24.1 g / 2.016 g/mol = 11.95 mol
Step 3: Use the stoichiometry of the reaction to determine the moles of H2SO4 required.
According to the balanced equation, 2 moles of Al react with 3 moles of H2SO4 to produce 3 moles of H2.
Therefore, the molar ratio of H2SO4 to H2 is 3:3 or 1:1.
Since the ratio is 1:1, we need the same number of moles of H2SO4 as moles of H2.
Moles of H2SO4 = 11.95 mol
Step 4: Calculate the volume of 5.0M H2SO4 solution needed.
Given that the concentration of the H2SO4 solution is 5.0M, which means it contains 5.0 moles of H2SO4 in 1 liter of solution.
We can use the formula: Moles = Volume (L) × Concentration (M)
Rearranging the formula to solve for Volume:
Volume (L) = Moles / Concentration (M)
Volume (L) = 11.95 mol / 5.0 M = 2.39 L
Therefore, the minimum amount of 5.0M H2SO4 necessary to produce 24.1g of H2(g) is 2.39 liters.