There are 1.2 x 10^24 atoms of carbon in a sample of aluminum acetate, Al(C2H3O2)3. How many moles of hydrogen are in the sample?
[?] moles H
To determine the number of moles of hydrogen in the sample, we need to know the ratio of hydrogen atoms to carbon atoms in aluminum acetate.
The molecular formula for aluminum acetate is Al(C2H3O2)3. From the formula, we can see that there are 3 hydrogen atoms for every 1 molecule of aluminum acetate.
Since we are given the number of carbon atoms in the sample (1.2 x 10^24 atoms), we can calculate the number of hydrogen atoms in the sample as follows:
Number of hydrogen atoms = Number of carbon atoms × (3 H atoms / 1 molecule of aluminum acetate)
= 1.2 x 10^24 atoms × (3 H atoms / 1 molecule of aluminum acetate)
Next, we need to convert the number of hydrogen atoms to moles. To do this, we need to know Avogadro's number, which is approximately 6.022 x 10^23 mol^-1.
Number of moles of hydrogen = Number of hydrogen atoms / Avogadro's number
= (1.2 x 10^24 atoms × 3) / 6.022 x 10^23 atoms/mol
Simplifying the expression:
Number of moles of hydrogen = (3.6 x 10^24 atoms) / (6.022 x 10^23 atoms/mol)
= 5.98 moles
Therefore, there are approximately 5.98 moles of hydrogen in the sample.
To determine the number of moles of hydrogen (H) in the sample, we first need to find the number of moles of aluminum acetate (Al(C2H3O2)3), and then multiply it by the ratio of moles of hydrogen to moles of aluminum acetate.
The chemical formula of aluminum acetate is Al(C2H3O2)3. From the formula, we can see that there are 3 hydrogen atoms (H) per molecule of aluminum acetate.
To find the moles of aluminum acetate, we need to convert the given number of atoms of carbon (1.2 x 10^24 atoms) to moles. We will use Avogadro's number, which is 6.022 x 10^23 atoms per mole.
Step 1: Calculate the moles of aluminum acetate
Number of moles of aluminum acetate = Number of atoms of carbon / Avogadro's number
Number of moles of aluminum acetate = (1.2 x 10^24 atoms) / (6.022 x 10^23 atoms/mol)
Calculating this gives us:
Number of moles of aluminum acetate = 1.99 moles
Step 2: Calculate the moles of hydrogen
Number of moles of hydrogen = Number of moles of aluminum acetate x 3 (since there are 3 hydrogen atoms per molecule of aluminum acetate)
Number of moles of hydrogen = 1.99 moles x 3
Calculating this gives us:
Number of moles of hydrogen = 5.97 moles
Therefore, there are approximately 5.97 moles of hydrogen in the sample of aluminum acetate.
To find the number of moles of hydrogen in the sample of aluminum acetate, we first need to determine the molar ratio of hydrogen to aluminum acetate.
Let's start by calculating the molar mass of aluminum acetate, Al(C2H3O2)3.
Aluminum (Al) has a molar mass of 26.98 g/mol.
Carbon (C) has a molar mass of 12.01 g/mol.
Hydrogen (H) has a molar mass of 1.01 g/mol.
Oxygen (O) has a molar mass of 16.00 g/mol.
So, the molar mass of aluminum acetate is:
(1 × 26.98 g/mol) + (6 × 12.01 g/mol) + (6 × 1.01 g/mol) + (18 × 16.00 g/mol) = 204.23 g/mol.
Now, let's calculate the number of moles of hydrogen using the given number of carbon atoms and the molar ratio.
The molar ratio of hydrogen to aluminum acetate can be determined from the chemical formula: Al(C2H3O2)3. We can see that for every 3 moles of aluminum acetate, there are 6 moles of hydrogen.
So, to calculate the number of moles of hydrogen, we'll use the following formula:
moles of H = (moles of Al(C2H3O2)3) × (moles of H / moles of Al(C2H3O2)3)
Given that there are 1.2 x 10^24 atoms of carbon in the sample, we can find the number of moles of aluminum acetate:
moles of Al(C2H3O2)3 = (number of carbon atoms) / (Avogadro's number) × (molar mass of Al(C2H3O2)3)
Number of carbon atoms = 1.2 x 10^24 atoms
Avogadro's number = 6.022 × 10^23 atoms/mol
moles of Al(C2H3O2)3 = (1.2 x 10^24) / (6.022 × 10^23) × 204.23 g/mol
After calculating the moles of aluminum acetate, we can find the moles of hydrogen:
moles of H = (moles of Al(C2H3O2)3) × (6 moles of H / 3 moles of Al(C2H3O2)3)
Now you can substitute the values into the equation and calculate the final answer.