30g of TiCl4 is mixed with 18g of water to from TiO2 and HCl. Write the chemical reaction and balance it.How much TiO2 is produced.
my answer:
TiCl4+2H2O= TiO2+4HCl
TiCl4+2H2O=TiO2+4HCl
The equation is ok.
This is a limiting reagent (LR) problem and you know that because amounts are given for both reactants.
mols TiCl4 = grams/molar mass = ?
mols H2O = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols TiCl4 to mols product. Do the same for mols H2O to mols product. It is likely these two values will not agree which means one is not right;the correct value in LR problems is ALWAYS the smaller value and the reagent producing that value is the LR.
Now convert that smaller value to grams product by grams = mols x molar mass = ?
To balance the chemical equation, you need to ensure that the number of atoms of each element is equal on both sides of the equation. Here's how you can balance it:
TiCl4 + 2H2O → TiO2 + 4HCl
On the left side, we have 1 Ti, 4 Cl, 2 H, and 2 O atoms.
On the right side, we have 1 Ti, 2 O, 4 H, and 1 Cl atoms.
To balance the chlorine (Cl) atoms, we need to add a coefficient of 4 in front of HCl:
TiCl4 + 2H2O → TiO2 + 4HCl
Now, let's calculate the amount of TiO2 produced.
From the balanced equation, we can see that the stoichiometric ratio between TiCl4 and TiO2 is 1:1. This means that for every mole of TiCl4 reacted, we will obtain one mole of TiO2.
First, let's convert the given masses of TiCl4 and water into moles using their molar masses:
30g TiCl4 × (1mol TiCl4 / 189.68g TiCl4) = 0.1582 mol TiCl4
18g H2O × (1mol H2O / 18.02g H2O) = 1.00 mol H2O
Since the stoichiometric ratio is 1:1, the moles of TiO2 produced will be equal to the moles of TiCl4 reacted:
Moles of TiO2 = 0.1582 mol
Therefore, 0.1582 moles of TiO2 will be produced.