if 5.00g magnesium is combined with 10.0 g of chlorine, show by calculation which substance is the limiting reactant and calculate the theoretical yield of magnesium chloride for the reaction. Someone PLEASE HELP ME!!!!

Mg + Cl2 -> MgCl2

5.00 g Mg / 24 g/mol / 1 (from balanced equation) = 0.21

10.0 g Cl2 / 71 g/mol / 2 (from balanced equation) = 0.070

Smallest number is limiting reactant = Cl2

Yield = 10.0 g Cl2 / 71g/mol X 1 mol MgCl2/1 mol Cl2 X 95 g MgCl2/mol = 13.4 g

10 g Cl2 / 71 g/mol /1 (balanced equation) = 0.141

Still the limiting reactant\
MgCl2 is still 13.4

Sorry!

On what

Well, well, well, looks like we've got a chemistry problem here! Fear not, my friend, I'll help you through this!

To determine the limiting reactant, we need to see which reactant is completely consumed first.

First, let's convert the masses of both magnesium and chlorine to moles:

Magnesium (Mg):
Molar mass of Mg = 24.31 g/mol
Number of moles of Mg = mass of Mg / molar mass of Mg
Number of moles of Mg = 5.00 g / 24.31 g/mol

Chlorine (Cl2):
Molar mass of Cl2 = 70.9 g/mol
Number of moles of Cl2 = mass of Cl2 / molar mass of Cl2
Number of moles of Cl2 = 10.0 g / 70.9 g/mol

Now, let's compare the moles of both reactants. The balanced equation for the reaction is:

Mg + Cl2 -> MgCl2

According to the balanced equation, the stoichiometric ratio of magnesium to chlorine is 1:1. So, whichever reactant has the smaller number of moles will be the limiting reactant.

Now it's time for the big reveal:

Moles of Mg = 5.00 g / 24.31 g/mol
Moles of Cl2 = 10.0 g / 70.9 g/mol

Now, compare the moles of both reactants. If the moles of magnesium are less than the moles of chlorine, then magnesium is the limiting reactant. If the moles of magnesium are more significant, then chlorine is the limiting reactant. Drumroll, please...

*Drumroll*

Who's the winner? Is it magnesium, or is it chlorine? Come on, tell me, I'm on the edge of my seat!

In this case, since the number of moles of Mg is less than the number of moles of Cl2, magnesium is the limiting reactant! Cue the confetti!

Now it's time to find the theoretical yield of magnesium chloride. According to the balanced equation, one mole of magnesium reacts with one mole of chlorine to produce one mole of magnesium chloride.

Since magnesium is the limiting reactant, the number of moles of magnesium chloride formed will be equal to the number of moles of magnesium used.

Theoretical yield of MgCl2 = Number of moles of Mg x molar mass of MgCl2

Don't worry, I'll do the math for you:

Theoretical yield of MgCl2 = (5.00 g / 24.31 g/mol) x (95.21 g/mol)

Now, all that's left is plugging those numbers in and calculating the answer. Take it away, calculator!

To determine the limiting reactant and calculate the theoretical yield of magnesium chloride, we first need to balance the chemical equation for the reaction.

The balanced equation for the reaction between magnesium and chlorine to form magnesium chloride is:

2Mg + Cl2 → 2MgCl2

Now, let's calculate the moles of each reactant:

Moles of magnesium (Mg) = mass / molar mass
Moles of magnesium = 5.00 g / 24.31 g/mol (molar mass of Mg)
Moles of magnesium = 0.2053 mol (round to 4 decimal places)

Moles of chlorine (Cl2) = mass / molar mass
Moles of chlorine = 10.0 g / 70.90 g/mol (molar mass of Cl2)
Moles of chlorine = 0.141 mol (round to 3 decimal places)

According to the balanced equation, the stoichiometric ratio between magnesium and chlorine is 2:1. This means that 2 moles of magnesium react with 1 mole of chlorine to produce 2 moles of magnesium chloride.

To determine the limiting reactant, we need to compare the moles of magnesium and chlorine in the reaction. Since the stoichiometric ratio is 2:1, we need to divide the moles of each reactant by their respective stoichiometric coefficients.

Moles of magnesium in ratio with chlorine = 0.2053 mol / 2 = 0.10265 mol (round to 5 decimal places)
Moles of chlorine in ratio with magnesium = 0.141 mol / 1 = 0.141 mol (round to 3 decimal places)

From the above calculations, we can see that magnesium is the limiting reactant because it produces fewer moles of product compared to chlorine. In other words, there is not enough magnesium to react completely with the available chlorine.

Now, let's calculate the theoretical yield of magnesium chloride:

Since 2 moles of magnesium react with 2 moles of magnesium chloride, we can use the moles of magnesium as the basis for calculating the theoretical yield.

Theoretical yield of magnesium chloride = moles of magnesium x molar mass of MgCl2
Theoretical yield of magnesium chloride = 0.10265 mol x (24.31 g/mol + 2*35.45 g/mol) (molar mass of MgCl2)
Theoretical yield of magnesium chloride = 0.10265 mol x 95.21 g/mol
Theoretical yield of magnesium chloride = 9.763 g (round to 3 decimal places)

Therefore, the theoretical yield of magnesium chloride for this reaction is 9.763 grams when 5.00 grams of magnesium are reacted with 10.0 grams of chlorine.