How many moles of TiCl4 can be produced when 9.00 mol Ti react with 4.00 mol Cl2?
I answered your first post.
Well, that's a mole-icious question! Let's take a clowny approach to it!
First, we need to balance the equation. The balanced equation for the reaction between titanium and chlorine is:
Ti + 2 Cl2 -> TiCl4
According to the equation, we see that for every one mole of titanium (Ti), we need two moles of chlorine gas (Cl2) to produce one mole of titanium tetrachloride (TiCl4).
Since we have 9.00 moles of titanium (Ti), and the stoichiometry tells us that we need a 1:2 ratio of Ti to Cl2, we need double the moles of chlorine gas.
So, for every one mole of titanium, we need two moles of chlorine gas. Thus, we need 2 * 9.00 = 18.00 moles of chlorine gas (Cl2).
Now, we have 4.00 moles of chlorine gas, which is less than what we need (18.00 moles). Therefore, the limiting reagent in this reaction is chlorine gas (Cl2).
Since chlorine gas is the limiting reagent, we can only produce the same number of moles of titanium tetrachloride as we have chlorine gas. Therefore, we can only produce 4.00 moles of titanium tetrachloride (TiCl4).
So, to answer your question, 4.00 moles of TiCl4 can be produced when 9.00 mol Ti react with 4.00 mol Cl2.
To determine the number of moles of TiCl4 that can be produced when 9.00 mol Ti reacts with 4.00 mol Cl2, we need to use the balanced chemical equation for the reaction.
The balanced equation for the reaction between Ti and Cl2 to produce TiCl4 is:
Ti + 2Cl2 -> TiCl4
From the reaction equation, we can see that 1 mol of Ti reacts with 2 mol of Cl2 to produce 1 mol of TiCl4.
Therefore, the molar ratio between Ti and TiCl4 is 1:1. This means that for every 1 mol of Ti, we can produce 1 mol of TiCl4.
Given that there are 9.00 mol of Ti, we can conclude that we can produce 9.00 mol of TiCl4.
Thus, 9.00 mol of TiCl4 can be produced when 9.00 mol Ti reacts with 4.00 mol Cl2.
To determine the number of moles of TiCl4 that can be produced, we need to determine the limiting reactant.
1. Start by writing and balancing the chemical equation for the reaction:
Ti + 2 Cl2 -> TiCl4
2. Calculate the number of moles of TiCl4 that can be produced from the number of moles of Ti:
9.00 mol Ti * (1 mol TiCl4 / 1 mol Ti) = 9.00 mol TiCl4
3. Calculate the number of moles of TiCl4 that can be produced from the number of moles of Cl2:
4.00 mol Cl2 * (1 mol TiCl4 / 2 mol Cl2) = 2.00 mol TiCl4
4. The limiting reactant is the reactant that produces the smaller amount of product. In this case, Cl2 is the limiting reactant because it produces only 2.00 moles of TiCl4, compared to 9.00 moles produced by Ti.
Therefore, when 9.00 mol Ti reacts with 4.00 mol Cl2, the maximum amount of TiCl4 that can be produced is 2.00 moles.