# chemisty help

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.

1. 👍 0
2. 👎 0
3. 👁 521
1. 8.1

1. 👍 0
2. 👎 0
posted by Anonymous

## Similar Questions

1. ### Chemistry

For the reaction shown, compute the theoretical yield of the product (in grams) Ti(s)+2Fe(g) = TiF2(s) 6.0 g Ti, 6.0g F2

asked by Lisa on November 1, 2010
2. ### Chemistry

For the reaction shown, compute the theoretical yield of the product in grams for each of the following initial amounts of reactancts 2Al(s) + 3Cl2(g) = 2AlCl3(s)

asked by Tanya on July 12, 2009
3. ### math

how do you calculate theoretical yield of something? I don't know where to find the formula You go to the balanced chemical equation, and look at the mole ratio between the reactants and products. The theoretical yield is the

asked by james on January 31, 2007
4. ### Chemistry

For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s) +3 Cl2(g) ---> 2 AlCl3(s) A. 2.5gAl , 2.5g Cl2 B. 7.7 g Al , 25.2 g Cl2 C. 0.240 g Al ,

asked by anonymous on February 11, 2009
5. ### Chemistry

For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s) +3 Cl2(g) ---> 2 AlCl3(s) A. 2.5gAl , 2.5g Cl2 B. 7.7 g Al , 25.2 g Cl2 C. 0.240 g Al ,

asked by anonymous on February 11, 2009
6. ### chem

Forty-two grams of benzoic acid is treated with concentrated nitric acid in some sulfuric acid. Forty-two grams of the major expected organic product is isolated. What is the percentage yield for this experiment? Give an equation

asked by Damon on August 6, 2007
7. ### chemistry

The theoretical yield of a reaction is 78.5 grams of product and the actual yield is 66.3 grams. What is the percent yield?

asked by Anonymous on December 11, 2012
8. ### Chem

How are these values used to determine percent? actual yield is quantity of a product found to be formed in a chemical reaction and theoretical yield is the amount of product predicted theoretical yield is larger because in

asked by Gregg on July 18, 2010
9. ### Chemistry Pretest

Fe can be prepared as 2 Al + Fe2O3 ----> 2 Fe + Al2O3. Suppose that 0.450 moles of Fe2O3 are reacted with an excess of Al. Suppose that 43.6 grams of Fe are obtained. What is the percent yield of Fe? a) 16.2% b) 60.7% c) 86.7% d)

asked by Sarah on September 28, 2012
10. ### Chemistry

I have a problem that has been driving me crazy trying to solve, and I was wondering if someone could help. The problem is this: "Given the reaction: CuSO4 + 4 NH3 ----> Cu(NH3)4SO4, if 10 grams of CuSO4 reacts with 30 grams of

asked by Josh on August 23, 2007
11. ### Chemistry 130

Will someone help me by letting me know if I did these correct, or if there the correct answers? Thanks! 2 (10). If two moles of hydrogen gas (H2) react in the following equation, how many moles of H2O will be formed? 2H2 + O2

asked by Jessie on September 8, 2009

More Similar Questions