a 0.2000 grams sample of aluminum metal is added to a solution containing 1.0000grams of an unknown compound made of platinum and chloride ion. the reaction results in the formation of aluminum chloride and platinum metal. when the reaction is complete, unreacted aluminum remains and this unreacted aluminum is consumed by reaction with hydrochloric acid. after washing and drying the, the mass of platinum metal is recovered is 0.5780.
what is the balanced equation for the reaction of aluminum with the original unknown compound?
what is the minimum mass of the aluminum metal needed to react with the platinum chloride compound?
also, what is the experimental percent of platinum in the original compound?
The problem doesn't say that the 1.00 g sample is pure; I'll assume it is.
mols Pt = 0.5780/195 = about 0.00296 but you need to do ALL of these calculations more carefully.
g Cl = 1.00-0.5760 = 0.422g and convert to mols = approx 0.012
So the empirical formula is PtCl4.
Equation is
4Al + 3PtCl4 ==> 4AlCl3 + 3Pt
mols Pt = 0.00296
mols Al = 0.00296 x (4 mola Al/3 mols Pt) = about 0.004 mols Al and that x atomic mass Al gives about 0.1 g Al as the minimum mass. Again you should redo all of this.
%Pt (if the compound is a pure compound) is (0.5780/1.00)*100 = ?
To deduce the balanced equation for the reaction of aluminum with the original unknown compound, let's start by identifying the reactants and products.
Reactants:
1. Aluminum metal (Al)
2. Unknown compound containing platinum and chloride ions
Products:
1. Aluminum chloride (AlCl₃)
2. Platinum metal (Pt)
Balancing the equation:
Since aluminum (Al) is a group 13 element, it has a charge of +3 when it's ionized. On the other hand, chloride ion (Cl⁻) has a charge of -1. To balance charges, we need three chloride ions for each aluminum atom.
The balanced equation for the reaction of aluminum with the original unknown compound is:
2 Al + 3 PtCl₄ → 2 AlCl₃ + 3 Pt
Now let's calculate the minimum mass of aluminum required to react with the platinum chloride compound.
From the balanced equation, we can see that the ratio of aluminum (Al) to platinum chloride (PtCl₄) is 2:3.
Given:
Mass of aluminum = 0.2000 grams
Mass of recovered platinum metal = 0.5780 grams
To find the minimum mass of aluminum, we can use the following ratio:
(0.2000 grams Al) / (2 grams Al) = (0.5780 grams Pt) / (3 grams PtCl₄)
Cross multiplying and solving for the missing quantity gives us:
(0.2000 grams Al) * (3 grams PtCl₄) = (0.5780 grams Pt) * (2 grams Al)
0.6000 grams PtCl₄ = 1.1560 grams Al
Therefore, the minimum mass of aluminum required to react with the platinum chloride compound is approximately 1.1560 grams.
To determine the balanced equation for the reaction of aluminum with the unknown compound, we need to understand the reactions involved.
Step 1: Reacting aluminum with the unknown compound:
Aluminum reacts with the chloride ions from the unknown compound to form aluminum chloride and platinum metal. We can represent this reaction as follows:
2Al + 3PtCl4 → 2AlCl3 + 3Pt
The coefficients are determined by ensuring that the equation follows the law of conservation of mass. In this balanced equation, we have 2 aluminum atoms reacting with 3 platinum chloride molecules to produce 2 molecules of aluminum chloride and 3 platinum metal atoms.
Now, let’s move on to determining the minimum mass of aluminum metal needed to react with the platinum chloride compound.
Step 2: Finding the moles of platinum:
You are given that the mass of platinum recovered is 0.5780 grams. To find the moles of platinum, divide this mass by the molar mass of platinum (195.08 g/mol):
Moles of platinum = 0.5780 g / 195.08 g/mol
Step 3: Finding the moles of aluminum:
According to the balanced equation, the ratio between aluminum and platinum is 2:3. Therefore, the moles of aluminum are found using the mole ratio:
Moles of aluminum = (2/3) * moles of platinum
Step 4: Calculating the mass of aluminum:
To find the mass of aluminum, multiply the moles of aluminum by the molar mass of aluminum (26.98 g/mol):
Mass of aluminum = Moles of aluminum * 26.98 g/mol
By following these steps, you can determine the balanced equation and the minimum mass of aluminum needed to react with the platinum chloride compound in this scenario.