Calculate the maximum number of moles and grams of iodic acid (HIO3) that can form when 632 g iodine trichloride reacts with 117.6 g of water.
The correct answer and explanation is :
To determine the maximum number of moles and grams of iodic acid (HIO₃) that can form when iodine trichloride (ICl₃) reacts with water, follow these steps:
Step 1: Write the Balanced Chemical Equation
[
ICl_3 + H_2O \rightarrow HIO_3 + HCl
]
From this equation, 1 mole of ICl₃ reacts with 1 mole of H₂O to form 1 mole of HIO₃ and 3 moles of HCl.
Step 2: Determine the Molar Mass of Each Substance
- ICl₃:
- Iodine (I) = 126.90 g/mol
- Chlorine (Cl) = 35.45 g/mol × 3 = 106.35 g/mol
- Molar mass of ICl₃ = 126.90 + 106.35 = 233.25 g/mol
- H₂O:
- Hydrogen (H) = 1.008 g/mol × 2 = 2.016 g/mol
- Oxygen (O) = 16.00 g/mol
- Molar mass of H₂O = 18.016 g/mol
- HIO₃:
- Hydrogen (H) = 1.008 g/mol
- Iodine (I) = 126.90 g/mol
- Oxygen (O) = 16.00 g/mol × 3 = 48.00 g/mol
- Molar mass of HIO₃ = 1.008 + 126.90 + 48.00 = 175.91 g/mol
Step 3: Determine the Moles of Reactants
- Moles of ICl₃:
[
\frac{632 \text{ g}}{233.25 \text{ g/mol}} = 2.71 \text{ moles}
] - Moles of H₂O:
[
\frac{117.6 \text{ g}}{18.016 \text{ g/mol}} = 6.53 \text{ moles}
]
Step 4: Identify the Limiting Reactant
Since the reaction follows a 1:1 mole ratio, compare the available moles:
- ICl₃ available = 2.71 moles
- H₂O available = 6.53 moles
Since ICl₃ is present in fewer moles, it is the limiting reactant.
Step 5: Determine the Maximum Amount of HIO₃ Produced
Because 1 mole of ICl₃ produces 1 mole of HIO₃, the moles of HIO₃ formed are equal to the moles of ICl₃ reacted:
[
\text{Moles of HIO₃} = 2.71 \text{ moles}
]
Convert to grams:
[
2.71 \text{ moles} \times 175.91 \text{ g/mol} = 477.0 \text{ g of HIO₃}
]
Final Answer
- Maximum moles of HIO₃ formed = 2.71 moles
- Maximum mass of HIO₃ formed = 477.0 g
Here is an image visually summarizing the reaction of iodine trichloride (ICl₃) with water (H₂O) to form iodic acid (HIO₃) and hydrochloric acid (HCl). The diagram includes molecular structures, the balanced equation, and a depiction of ICl₃ as the limiting reactant.