Doesn't mean it's wrong. In fact it can answer scientific questions very well.
For example:
Question:
If I added 3.57gr of malic acid to a 1 liter soda bottle with a magnesium rod in it and filled it up with 5 degree Celsius water, what would the pressure inside the bottle be and how much hydrogen would be dissolved in the water? Also, what other chemicals would be present and at what concentration?
Answer:
- Reaction: C4H6O5 (malic acid) + 5Mg + 5H2O → 5Mg(OH)2 + C4H4MgO5 + 5H2
- Calculate moles of malic acid: 3.57g / 134.09 g/mol = 0.02662 mol
- Hydrogen produced: 0.02662 mol malic acid × 5 mol H2 / 1 mol malic acid = 0.1331 mol H2
- Pressure calculation: Using ideal gas law: PV = nRTP = nRT / VP = (0.1331 mol × 0.08206 L⋅atm/mol⋅K × 278K) / 1LP ≈ 3.03 atm or 307 kPa
- Dissolved hydrogen: Using Henry's law: C = kPk for H2 at 5°C ≈ 8.7 × 10^-4 mol/L⋅atmC = 8.7 × 10^-4 mol/L⋅atm × 3.03 atm = 0.00264 mol/L
- Mass of dissolved H2 = 0.00264 mol/L × 2.016 g/mol = 0.00532 g/L or 5.32 mg/L
- Other chemicals present:
a) Magnesium hydroxide (Mg(OH)2):0.02662 mol × 5 = 0.1331 mol
Mass = 0.1331 mol × 58.32 g/mol = 7.76 g
Concentration = 7.76 g/L
b) Magnesium malate (C4H4MgO5):0.02662 mol
Mass = 0.02662 mol × 172.37 g/mol = 4.59 g
Concentration = 4.59 g/L
c) Unreacted magnesium (if rod is in excess)
- Final solution composition:
- Dissolved hydrogen: 5.32 mg/L
- Magnesium hydroxide: 7.76 g/L (mostly as a precipitate)
- Magnesium malate: 4.59 g/L (dissolved)
- Pressure: 3.03 atm or 307 kPa
- pH: Basic due to Mg(OH)2 formation