When 5.49 g of platinum reacts with an excess of fluorine, 7.65 g of platinum(_) fluoride forms.
a.
What is the mass of fluorine in the compound?
b. Find the number of moles of platinum that reacted.
c. Find the number of moles of fluorine that reacted.
d. Calculate the ratio of moles of F to moles Pt that reacted. Be sure to use the appropriate number of significant figures. Give the empirical formula of platinum( ) fluoride: PtF?. Write the correct name for the compound.
The second part is this.
The theoretical value for the ration of moles of F to moles of Pt is (exactly) 4. Calculate the percent error for the experimental value found in 3d.
......Pt + F2 ==> PtFx
.....5.49..xs......7.65
a. PtFx weighs 7.65. Pt weighs 5.49. So mass F must be ?
b & c. mols = grams/molar mass
d. Calculate mols F to 1 mol Pt.
Show your work and explain what you don't understand if you get stuck.
To solve this problem, we can follow these steps:
a. Calculate the mass of fluorine in the compound:
Given:
- Mass of platinum: 5.49 g
- Mass of platinum fluoride: 7.65 g
First, we subtract the mass of platinum from the mass of platinum fluoride to find the mass of fluorine:
Mass of fluorine = Mass of platinum fluoride - Mass of platinum
Mass of fluorine = 7.65 g - 5.49 g
Mass of fluorine = 2.16 g
Therefore, the mass of fluorine in the compound is 2.16 g.
b. Find the number of moles of platinum that reacted:
To find the number of moles, we divide the mass of platinum by its molar mass.
The molar mass of platinum (Pt) is 195.08 g/mol.
Number of moles of platinum = Mass of platinum / Molar mass of platinum
Number of moles of platinum = 5.49 g / 195.08 g/mol
Using a calculator, we find that the number of moles of platinum is approximately 0.0282 moles.
c. Find the number of moles of fluorine that reacted:
To find the number of moles, we divide the mass of fluorine by its molar mass.
The molar mass of fluorine (F) is 18.9984 g/mol.
Number of moles of fluorine = Mass of fluorine / Molar mass of fluorine
Number of moles of fluorine = 2.16 g / 18.9984 g/mol
Using a calculator, we find that the number of moles of fluorine is approximately 0.113 moles.
d. Calculate the ratio of moles of F to moles of Pt that reacted:
To calculate the ratio of moles of fluorine to moles of platinum, we divide the number of moles of fluorine by the number of moles of platinum.
Ratio = Moles of F / Moles of Pt
Ratio = 0.113 moles / 0.0282 moles
Ratio = 4
The ratio is 4.
The empirical formula of platinum( ) fluoride is PtF4.
The correct name for the compound is platinum tetrafluoride.
To answer these questions, we need to use the given information about the reaction between platinum and fluorine and apply the principles of stoichiometry. Stoichiometry is the calculation of quantities in chemical reactions based on balanced equations.
a. To find the mass of fluorine in the compound, we need to subtract the mass of platinum present from the total mass of the platinum fluoride formed.
Mass of platinum fluoride = 7.65 g
Mass of platinum = 5.49 g
Mass of fluorine = Mass of platinum fluoride - Mass of platinum
Mass of fluorine = 7.65 g - 5.49 g
Mass of fluorine = 2.16 g
Therefore, the mass of fluorine in the compound is 2.16 g.
b. To find the number of moles of platinum that reacted, we need to convert the mass of platinum to moles using the molar mass of platinum.
Molar mass of platinum = 195.08 g/mol
Number of moles of platinum = Mass of platinum / Molar mass of platinum
Number of moles of platinum = 5.49 g / 195.08 g/mol
Number of moles of platinum ≈ 0.0282 mol (rounded to four significant figures)
Therefore, the number of moles of platinum that reacted is approximately 0.0282 mol.
c. To find the number of moles of fluorine that reacted, we need to divide the number of moles of platinum fluoride formed by the stoichiometric coefficient of fluorine in the balanced equation.
The balanced equation for the reaction between platinum and fluorine is:
Pt + F2 -> PtF4
From the equation, we can see that the stoichiometric coefficient of fluorine is 2, meaning two moles of fluorine react with one mole of platinum.
Number of moles of fluorine = (Number of moles of platinum fluoride) × (Stoichiometric coefficient of fluorine)
Number of moles of fluorine = 0.0282 mol × 2
Number of moles of fluorine = 0.0564 mol
Therefore, the number of moles of fluorine that reacted is 0.0564 mol.
d. To calculate the ratio of moles of fluorine to moles of platinum that reacted, we divide the moles of fluorine by the moles of platinum.
Ratio of moles of F to moles Pt = (Number of moles of fluorine) / (Number of moles of platinum)
Ratio of moles of F to moles Pt = 0.0564 mol / 0.0282 mol
Ratio of moles of F to moles Pt ≈ 2.00 (rounded to two significant figures)
Therefore, the ratio of moles of F to moles Pt that reacted is approximately 2.00.
The empirical formula of platinum fluoride is PtF4, as indicated in the balanced equation. A balanced equation shows the ratio of elements in a compound, and in this case, it tells us that there are four moles of fluorine for every one mole of platinum.
The correct name for the compound PtF4 is platinum(IV) fluoride. The Roman numeral 'IV' indicates the charge of the platinum ion in the compound (since fluorine has a fixed charge of -1).