Two different chloride compounds of platinum are known, compound X and Y. When 3.45g of compound X is heated, 2.72g of compound Y is formed to 1.99g of platinum metal and some more chlorine gas. Determine the formulas of compounds X and Y.

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To determine the formulas of compounds X and Y, we need to analyze the information given and calculate the molar ratios.

Let's start by calculating the number of moles of each substance involved.

1) Moles of compound X:
Molar mass of X = ?
Mass of X = 3.45 g

To find the molar mass of X, we need to know the periodic table values. Without the periodic table values, we cannot calculate the molar mass of compound X.

To determine the formulas of compounds X and Y, we need to use the law of conservation of mass. According to this law, the total mass of the reactants should be equal to the total mass of the products in a chemical reaction.

Let's start by assigning variables to the unknowns:

- Let's assume the formula of compound X is PtClₓ, where x is the unknown subscript representing the number of chlorine atoms bonded to platinum.
- Similarly, let's assume the formula of compound Y is PtClᵧ, where y is the unknown subscript representing the number of chlorine atoms bonded to platinum.

Using these assumptions, we can construct balanced equations for the reaction.

The reaction can be represented as follows:
PtClₓ → PtClᵧ + Pt + Cl₂

Now, let's write the mass balance equation for the reaction:
Mass of X = Mass of Y + Mass of Pt + Mass of Cl₂

We are given the following information:
Mass of X = 3.45 g
Mass of Y = 2.72 g
Mass of Pt = 1.99 g

Substituting these values into the mass balance equation, we get:
3.45 g = 2.72 g + 1.99 g + Mass of Cl₂

Rearranging the equation, we find:
Mass of Cl₂ = 3.45 g − 2.72 g − 1.99 g
= 0.54 g

Now, we need to convert the mass of Cl₂ to the number of moles using the molar mass of Cl₂, which is 70.91 g/mol.

Number of moles of Cl₂ = Mass of Cl₂ / Molar mass of Cl₂
= 0.54 g / 70.91 g/mol
= 0.0076 mol

Since Cl₂ is diatomic (contains two chlorine atoms), the number of moles of Cl atoms is twice the number of moles of Cl₂.

Number of moles of Cl atoms = 2 * Number of moles of Cl₂
= 2 * 0.0076 mol
= 0.0152 mol

Now, we can determine the values of x and y based on the number of moles of Cl atoms.

From the formula PtClₓ, we know that the number of moles of Cl atoms in compound X is x.
From the formula PtClᵧ, we know that the number of moles of Cl atoms in compound Y is y.

Given that the number of moles of Cl atoms is 0.0152 mol, we can equate it to the sum of x moles in compound X and y moles in compound Y:

0.0152 mol = x mol + y mol

To find the whole number values for x and y, we need to know the ratios between the moles of Cl in the two compounds. We can determine these ratios by comparing the masses of the compounds.

The mass of compound X (PtClₓ) is 3.45 g, and the mass of compound Y (PtClᵧ) is 2.72 g.

Since the molar mass of Cl is 35.45 g/mol and the molar mass of Pt is 195.08 g/mol, we can find the respective number of moles for each compound.

Number of moles of X = Mass of X / Molar mass of X
= 3.45 g / (195.08 g/mol + 35.45 g/mol) [Adding the molar masses of Pt and Cl]
= 0.0168 mol

Number of moles of Y = Mass of Y / Molar mass of Y
= 2.72 g / (195.08 g/mol + 35.45 g/mol) [Adding the molar masses of Pt and Cl]
= 0.0132 mol

We can then determine the ratio between the moles of Cl in compound X and compound Y as follows:

Ratio = Number of moles of Cl in X / Number of moles of Cl in Y
= x mol / y mol

Substituting the values we found earlier, we have:

Ratio = 0.0168 mol / 0.0132 mol
= 1.27

Since the ratio is close to 1, we can assume that both compounds have approximately the same number of chlorine atoms (x ≈ y).

Based on the information provided, the formulas of compounds X and Y can be determined as follows:

Compound X: PtClₓ, where x is approximately 1
Compound Y: PtClᵧ, where y is approximately 1

Therefore, the formulas of compounds X and Y are PtCl and PtCl.