What volume of Al metal have density 2.70 g/cm3 is required to produce o.752 g per mol of H2 gas by following reaction
2Al +6HCL ----- AlCl3+3H2
You have a typo or something.
o.752 g per mol of H2 gas
Makes no sense to me.
A mol of H2 is 2 grams because H has atomic mass of 1
If you want a mol of H2
You need 2/3 of a mol of Al
A mol of Al has mass of 27 grams
so
2/3 of 27 = 18 grams of Al
Remember, I do not know what your question is.
To find the volume of Al metal required, we need to use the balanced chemical equation and the concept of stoichiometry.
In the balanced chemical equation: 2Al + 6HCl -> 2AlCl3 + 3H2
Given:
Density of Al = 2.70 g/cm^3
Mass of H2 gas produced = 0.752 g/mol
Step 1: Find the molar mass of Al
The molar mass of Al can be found using its atomic mass on the periodic table, which is 26.98 g/mol.
Step 2: Calculate the number of moles of H2 gas produced
We have been given the mass of H2 gas produced, which is 0.752 g/mol. To convert this mass to moles, divide it by the molar mass of H2:
Number of moles = Mass / Molar mass
Number of moles = 0.752 g / 2.02 g/mol (molar mass of H2)
Number of moles = 0.372 mol
Step 3: Use stoichiometry to calculate the number of moles of Al required
From the balanced equation, we can see that 2 moles of Al produce 3 moles of H2 gas. So,
2 moles Al --> 3 moles H2 gas
x moles Al --> 0.372 moles H2 gas (from step 2)
To find the value of x:
x = (0.372 moles H2 gas * 2 moles Al) / 3 moles H2 gas
x = 0.248 mol
Step 4: Convert moles of Al to grams using the molar mass of Al
Mass of Al = Moles of Al * Molar mass of Al
Mass of Al = 0.248 mol * 26.98 g/mol
Mass of Al = 6.73 g
Step 5: Calculate the volume of Al by utilizing its density
Volume = Mass / Density
Volume = 6.73 g / 2.70 g/cm^3
Volume ≈ 2.49 cm^3
Therefore, approximately 2.49 cm^3 of Al metal is required to produce 0.752 g/mol of H2 gas.