To determine the formula mass, we sum the atomic masses of all atoms in the chemical formula. We will use the following approximate atomic masses:
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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To determine the formula mass, we sum the atomic masses of all atoms in the chemical formula. We will use the following approximate atomic masses:
N = 14.01 g/mol
H = 1.01 g/mol
Cl = 35.45 g/mol
Na = 22.99 g/mol
C = 12.01 g/mol
O = 16.00 g/mol
Fe = 55.85 g/mol
Al = 26.98 g/mol
S = 32.07 g/mol
a) $\text{NH}_4\text{Cl}$
Step 1: Identify the number of atoms for each element.
1 nitrogen (N) atom, 4 hydrogen (H) atoms, 1 chlorine (Cl) atom.
Step 2: Calculate the total mass.
$$ \text{Formula mass} = (1 \times 14.01) + (4 \times 1.01) + (1 \times 35.45) $$
$$ \text{Formula mass} = 14.01 + 4.04 + 35.45 $$
$$ \text{Formula mass} = 53.50 \text{ g/mol} $$
The formula mass of $\text{NH}_4\text{Cl}$ is $\boxed{\text{53.50 g/mol}}$.
b) $\text{NaHCO}_3$
Step 1: Identify the number of atoms for each element.
1 sodium (Na) atom, 1 hydrogen (H) atom, 1 carbon (C) atom, 3 oxygen (O) atoms.
Step 2: Calculate the total mass.
$$ \text{Formula mass} = (1 \times 22.99) + (1 \times 1.01) + (1 \times 12.01) + (3 \times 16.00) $$
$$ \text{Formula mass} = 22.99 + 1.01 + 12.01 + 48.00 $$
$$ \text{Formula mass} = 84.01 \text{ g/mol} $$
The formula mass of $\text{NaHCO}_3$ is $\boxed{\text{84.01 g/mol}}$.
c) $\text{FeCl}_3$
Step 1: Identify the number of atoms for each element.
1 iron (Fe) atom, 3 chlorine (Cl) atoms.
Step 2: Calculate the total mass.
$$ \text{Formula mass} = (1 \times 55.85) + (3 \times 35.45) $$
$$ \text{Formula mass} = 55.85 + 106.35 $$
$$ \text{Formula mass} = 162.20 \text{ g/mol} $$
The formula mass of $\text{FeCl}_3$ is $\boxed{\text{162.20 g/mol}}$.
d) $\text{C}_2\text{H}_5\text{OH}$
Step 1: Identify the number of atoms for each element.
2 carbon (C) atoms, 6 hydrogen (H) atoms (5 in $\text{C}_2\text{H}_5$ and 1 in OH), 1 oxygen (O) atom.
Step 2: Calculate the total mass.
$$ \text{Formula mass} = (2 \times 12.01) + (6 \times 1.01) + (1 \times 16.00) $$
$$ \text{Formula mass} = 24.02 + 6.06 + 16.00 $$
$$ \text{Formula mass} = 46.08 \text{ g/mol} $$
The formula mass of $\text{C}_2\text{H}_5\text{OH}$ is $\boxed{\text{46.08 g/mol}}$.
e) $\text{Al}_2(\text{SO}_4)_3$
Step 1: Identify the number of atoms for each element.
2 aluminium (Al) atoms, 3 sulfur (S) atoms (from $3 \times \text{S}$), 12 oxygen (O) atoms (from $3 \times 4 \times \text{O}$).
Step 2: Calculate the total mass.
$$ \text{Formula mass} = (2 \times 26.98) + (3 \times 32.07) + (12 \times 16.00) $$
$$ \text{Formula mass} = 53.96 + 96.21 + 192.00 $$
$$ \text{Formula mass} = 342.17 \text{ g/mol} $$
The formula mass of $\text{Al}_2(\text{SO}_4)_3$ is $\boxed{\text{342.17 g/mol}}$.
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