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.

Question

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.

if a 2.000 gram sample of the platinum chloride had been used, how many grams of chlorine would you expect it to contain?

Answer 1

A lot of verbiage, most which is unimportant.

.....PtClx ==> Pt + xCl2
I....1.00.....0.....0
E....-1.00..0.5780..(1.00-0.5780)
.......0....0.5780...0.422g

So if I used twice as much PtClx I would expect twice as much Cl2 or 0.844 g.

Answer 2

whats the balanced equation for the reaction of aluminum with the original unknown compound?

Answer 3

To find the number of grams of chlorine in the platinum chloride compound, we need to use the given information and some stoichiometry.

First, let's calculate the moles of aluminum used in the reaction:

Molar mass of aluminum (Al) = 26.98 g/mol

Moles of Al used = mass of Al sample / molar mass of Al
= 0.2000 g / 26.98 g/mol

Next, let's calculate the moles of platinum formed:

Molar mass of platinum (Pt) = unknown

Moles of Pt formed = mass of Pt recovered / molar mass of Pt
= 0.5780 g / molar mass of Pt

Now, we can establish a relationship between moles of platinum and moles of aluminum based on the balanced chemical equation. The equation tells us that 2 moles of Al react with 1 mole of PtCl2 to give 1 mole of Pt and 2 moles of AlCl3.

From this relationship, we can find the moles of PtCl2 used:

Moles of PtCl2 used = (2 moles of Al)/(1 mole of Pt)
= 2 * (moles of Al used)

Now, we can calculate the molar mass of PtCl2 using the given information. The molar mass is the mass of PtCl2 that contains 1 mole of Pt.

Molar mass of PtCl2 = mass of PtCl2 / moles of PtCl2

Finally, we can calculate the mass of chlorine in the PtCl2 compound:

Mass of chlorine = molar mass of PtCl2 - molar mass of Pt

Therefore, to answer the question, we need the molar mass of PtCl2. Unfortunately, it is not provided in the given information.