for the reaction shown, compute the theoretical yield of the product in grams for each of the following initial amounts of reactants.
Ti + 2F2 to make TiF4
There are 3 sub questions for this. Help me out with one, then I'll try to figure out the rest. thanks
a) 4.8g Ti; 3.2gF2
This is a limiting reagent problem. It is worked the same way as a regular stoichiometry problem is worked but with a twist or two.
Step1. Write the balanced equation.
Ti + 2F2 ==> TiF4
Step 2. Convert grams into mols.
3a. mols Ti = grams/atomic mass = 4.8/48 = 0.1 mol Ti
3b. mols F2 = 3.2g/38 = 0.084 mol F2.
Step 3. Using the coefficients in the balanced equation, convert mols in a and b of part 2 to mols of the product.
3a. convert mols Ti.
0.1 mol Ti x (1 mol TiF4/1 mol Ti) = 0.1 x 1/1 = 0.1 mol TiF4 produced.
3b. convert mols F2.
0.084 mol F2 x (1 mol TiF4/2 mols F2) = 0.084 x 1/2 = 0.0421 mol TiF4 produced.
3c. Obviously, both numbers can't be correct. The smaller of the two numbers of mols will be the correct one to use and that is the limiting reagent. Therefore, 0.0421 will be the mols TiF4 produced.
Step 4. Convert mols TiF4 to grams.
grams TiF4 = mols TiF4 x molar mass TiF4.
For a regular stoichiometry problem you won't have steps 2b or 3b or 3c. Everything else is the same.
You will need to go through this problem again because I just estimated the atomic masses of F2 and Ti. Post your work if you get stuck. Check my work. It's easy to make a typo when I'm in a hurry.
Step 1: Write the balanced equation
Ti + 2F2 -> TiF4
Step 2: Convert grams into moles
a) Ti
grams Ti = 4.8g
molar mass Ti = 48g/mol
moles Ti = grams Ti / molar mass Ti
moles Ti = 4.8g / 48g/mol
moles Ti = 0.1 mol Ti
b) F2
grams F2 = 3.2g
molar mass F2 = 38g/mol
moles F2 = grams F2 / molar mass F2
moles F2 = 3.2g / 38g/mol
moles F2 = 0.084 mol F2
Step 3: Convert moles of reactants to moles of product
a) Moles of Ti -> Moles of TiF4
moles TiF4 = moles Ti * (1 mol TiF4 / 1 mol Ti)
moles TiF4 = 0.1 * (1 mol TiF4 / 1 mol Ti)
moles TiF4 = 0.1 mol TiF4
b) Moles of F2 -> Moles of TiF4
moles TiF4 = moles F2 * (1 mol TiF4 / 2 mol F2)
moles TiF4 = 0.084 * (1 mol TiF4 / 2 mol F2)
moles TiF4 = 0.042 mol TiF4
Step 4: Determine the limiting reactant
The limiting reactant is the one that produces fewer moles of product. In this case, Ti produces 0.1 mol TiF4 and F2 produces 0.042 mol TiF4. Therefore, F2 is the limiting reactant.
Step 5: Calculate the theoretical yield of TiF4 in grams
moles TiF4 = 0.042 mol
molar mass TiF4 = 123.9g/mol
grams TiF4 = moles TiF4 * molar mass TiF4
grams TiF4 = 0.042 mol * 123.9g/mol
grams TiF4 = 5.20g
So, the theoretical yield of TiF4 is 5.20 grams.
To calculate the theoretical yield, we need to determine the limiting reactant. This is the reactant that will be completely consumed and determine the amount of product that can be formed.
In this case, we have 4.8g of Ti and 3.2g of F2.
Step 1: Write the balanced equation:
Ti + 2F2 -> TiF4
Step 2: Convert grams into moles:
Molar mass of Ti = 47.88 g/mol
Molar mass of F2 = 38.00 g/mol
Moles of Ti = 4.8g / 47.88 g/mol = 0.1 mol Ti
Moles of F2 = 3.2g / 38.00 g/mol = 0.084 moles F2
Step 3: Determine the limiting reactant:
To find the limiting reactant, we need to compare the moles of each reactant to the stoichiometric ratio in the balanced equation.
From the balanced equation, we can see that 1 mole of Ti reacts with 2 moles of F2 to produce 1 mole of TiF4.
For Ti:
0.1 mol Ti * (1 mol TiF4 / 1 mol Ti) = 0.1 mol TiF4
For F2:
0.084 mol F2 * (1 mol TiF4 / 2 mol F2) = 0.042 mol TiF4
Since we have less moles of TiF4 obtained from F2, F2 is the limiting reactant.
Step 4: Calculate the theoretical yield of TiF4 in grams.
To calculate the grams of TiF4, we need to convert moles of TiF4 to grams using its molar mass.
Molar mass of TiF4 = 63.87 g/mol
Theoretical yield of TiF4 = 0.042 mol TiF4 * 63.87 g/mol = 2.6934 g TiF4 (rounded to four decimal places)
Therefore, the theoretical yield of TiF4 is approximately 2.6934 grams for the given amounts of reactants.