Consider the following equation:

TiCl4(g) + 2Mg(l) → Ti(s) + 2MgCl2(l)
3.54×107g of TiCl4(g) are reacted completely. If 7.91×106g of Ti(s) is actually obtained, calculate the % yield.

I'm confused with the phases unless this reaction is occurring at an elevated temperature. At any rate

mols TiCl4 = grams/molar mass
Using the coefficients in the balanced equation, convert mols TiCl4 to mols Ti.
Now convert mols Ti to grams Ti by g Ti = mols Ti x atomic mass Ti. This is the theoretical yield (TY).
%yield = (actual yield/TY)*100 = ?

To find the percent yield, we need to compare the actual yield to the theoretical yield.

First, let's calculate the molar mass of TiCl4 and Ti to determine the stoichiometry of the reaction:

Molar mass of TiCl4:
Ti = 47.88 g/mol
Cl = 35.45 g/mol × 4 = 141.8 g/mol
Total molar mass = 47.88 g/mol + 141.8 g/mol = 189.7 g/mol

Molar mass of Ti:
Ti = 47.88 g/mol

Now, we can calculate the theoretical yield of Ti(s) using the following steps:

Step 1: Convert the given mass of TiCl4(g) to moles:
moles of TiCl4 = mass / molar mass
moles of TiCl4 = 3.54×10^7 g / 189.7 g/mol

Step 2: Use the stoichiometric ratios to calculate the moles of Ti(s):
From the balanced equation, we see that 1 mole of TiCl4 produces 1 mole of Ti.
moles of Ti = moles of TiCl4

Step 3: Convert the moles of Ti(s) to grams:
mass of Ti(s) = moles of Ti × molar mass
mass of Ti(s) = moles of Ti × 47.88 g/mol

Now, we can calculate the percent yield:

Percent yield = (Actual yield / Theoretical yield) × 100

Actual yield = 7.91×10^6 g
Theoretical yield = mass of Ti(s) calculated in Step 3

Percent yield = (7.91×10^6 g / Theoretical yield) × 100

Now, plug in the values and calculate the percent yield.