How many moles of TiCl4 can be produced when 9.00 mol Ti react with 4.00 mol Cl2?
This is a limiting reagent problem.
1. Write the equation and balance it.
2. Using the coefficients in the balanced equation, convert moles Ti to moles TiCl4.
3. Do the same procedure to convert moles Cl2 to moles TiCl4.
4. Likely, the answer to 2 will be different from the answer to 3. Obviously, one of them must be incorrect. The correct one in limiting reagent problems is ALWAYS the smaller value.
Well, I could give you a serious answer, but I'm more of a clown than a chemist. So instead, let's imagine TiCl4 as a really fancy dessert, like a gourmet cupcake. So, when 9.00 moles of Ti and 4.00 moles of Cl2 come together, it's like a big baking party!
Now, let's say each mole of Ti combines with 4 moles of Cl2 to make TiCl4 cupcakes. You know, because it's a fancy recipe. So, with 4.00 moles of Cl2, that means we have enough ingredients for 4 cupcakes, because 4 moles of Cl2 per cupcake.
But here's the fun part! We have 9.00 moles of Ti, and each mole of Ti makes one cupcake. So, we can make 9 cupcakes with that! However, even though we have enough Cl2 for only 4 cupcakes, we can't just leave the extra 5 cupcakes Ti-less. That would be cruel!
So, to make the best use of our ingredients, we can only make 4 cupcakes. Each cupcake needs 1 mole of Ti and 4 moles of Cl2. Therefore, the maximum number of moles of TiCl4 that can be produced is 4 moles. So, enjoy your 4 delicious TiCl4 cupcakes!
To determine the number of moles of TiCl4 that can be produced, we need to determine the limiting reactant first. The limiting reactant is the reactant that is completely consumed and limits the amount of product that can be formed.
To find the limiting reactant, we compare the moles of the reactants to the stoichiometric ratio in the balanced equation. The balanced equation for the reaction is:
Ti + 2Cl2 → TiCl4
From the balanced equation, we can see that 1 mole of Ti reacts with 2 moles of Cl2 to produce 1 mole of TiCl4.
Now, let's calculate the number of moles of TiCl4 that can be produced using the mole ratios:
Moles of TiCl4 = (moles of Ti) × (moles of TiCl4 / moles of Ti)
Moles of TiCl4 = 9.00 mol Ti × (1 mol TiCl4 / 1 mol Ti)
Moles of TiCl4 = 9.00 mol Ti
Since the moles of TiCl4 produced are equal to the moles of Ti, we can conclude that 9.00 moles of TiCl4 can be produced when 9.00 mol Ti reacts with 4.00 mol Cl2.
To determine the number of moles of TiCl4 produced, we need to use the balanced chemical equation and the stoichiometry of the reaction.
The balanced chemical equation for the reaction between Ti and Cl2 is:
Ti + 2Cl2 → TiCl4
From the balanced equation, we can see that for every 1 mole of Ti, 2 moles of Cl2 are required to produce 1 mole of TiCl4.
Given that we have 9.00 moles of Ti and 4.00 moles of Cl2, we need to determine the limiting reactant. The limiting reactant is the substance that is completely consumed, thus determining the maximum amount of product that can be formed.
To find the limiting reactant, we compare the moles of each reactant to the stoichiometric coefficients in the balanced equation:
For Ti: 9.00 mol Ti × (2 mol Cl2 / 1 mol Ti) = 18.00 mol Cl2
For Cl2: 4.00 mol Cl2
Theoretically, 18.00 mol Cl2 is required to react with all 9.00 mol of Ti. However, since we only have 4.00 mol of Cl2, it is the limiting reactant.
Using the stoichiometry of the balanced equation, we can determine the moles of TiCl4 produced from the limiting reactant:
4.00 mol Cl2 × (1 mol TiCl4 / 2 mol Cl2) = 2.00 mol TiCl4
Therefore, when 9.00 mol of Ti react with 4.00 mol of Cl2, the maximum amount of TiCl4 that can be produced is 2.00 moles.