Consider the folllowing chemical equation

TiCL4(g) + @Mg(i) --- Ti(s) + 2MgCl(i)
3.54 x 10 to powerof 7g of TiCl4(g) were reacted completely and 7.91 x 10 to pwer of 10 of Ti(s) was obtained in the experiment,
A) Calculate the theoretical yield of Ti(s)
b) What is the actual yield of Ti(s) in this experiment.
C) Calculate the % yield of Ti(s) in this experiement.

I don't know of any tutor here who knows what "UA" means, but I do know that "UA" is not a subject area.

What is this? Calculus? Statistics? What?

To calculate the theoretical yield of Ti(s):

Step 1: Determine the molar mass of TiCl4(g) and Ti(s)
- The molar mass of TiCl4 is calculated as follows:
Ti = 47.87 g/mol
Cl = 35.45 g/mol (4 Cl atoms)
Total molar mass of TiCl4 = (47.87 g/mol) + (4 * 35.45 g/mol) = 189.68 g/mol

- The molar mass of Ti is 47.87 g/mol

Step 2: Convert the given mass of TiCl4(g) to moles
- Divide the mass of TiCl4(g) by its molar mass:
Moles of TiCl4(g) = 3.54 x 10^7 g / 189.68 g/mol = 1.866 x 10^5 mol of TiCl4(g)

Step 3: Calculate the stoichiometric ratio between TiCl4(g) and Ti(s)
- From the balanced equation, we see that the ratio between TiCl4(g) and Ti(s) is 1:1.
- Therefore, the moles of Ti(s) will be the same as the moles of TiCl4(g):

Moles of Ti(s) = 1.866 x 10^5 mol of TiCl4(g)

Step 4: Calculate the theoretical yield of Ti(s)
- Multiply the moles of Ti(s) by its molar mass:
Theoretical yield of Ti(s) = (1.866 x 10^5 mol) * (47.87 g/mol) = 8.923 x 10^6 g

Therefore, the theoretical yield of Ti(s) is 8.923 x 10^6 g.

To calculate the actual yield of Ti(s), we use the given information that 7.91 x 10^10 g of Ti(s) was obtained in the experiment.

Therefore, the actual yield of Ti(s) is 7.91 x 10^10 g.

To calculate the percentage yield of Ti(s), use the following formula:

Percentage yield = (actual yield / theoretical yield) x 100

Substituting the values we calculated:

Percentage yield = (7.91 x 10^10 g / 8.923 x 10^6 g) x 100

Therefore, the percentage yield of Ti(s) is 887,513%.