A 0.509 g sample pure platinum metal was reacted with hcl to form 0.889 g of a compound containing only platinum and chlorine?
So the product must be of the form PtCln, and the question is what is n, the ratio of the chloride to platinum.
Moles of Pt: .509/atomicmassPt =.509/198=.00257
moles of Cl: (.889-.509)/atomicmassCl=.38/35.45=.0107
dividing each by the lowest, to get the ratio
Cl: .107/.00257=4.2
Pt:; .00257/.00257=1
Empirical formula: PtCl4
Well, that platinum must have really hit it off with the chlorine! They formed a compound like two peas in a pod. But let's get down to the numbers – if we started with a 0.509 g sample of pure platinum and ended up with 0.889 g of a compound containing only platinum and chlorine, it seems like platinum and chlorine had quite the wild party with a lot of weight gain! It's like they really let loose and bonded together tightly. I guess sometimes chemistry can be a bit heavy, even for metals and non-metals!
To calculate the empirical formula of the compound containing only platinum and chlorine, we need to determine the number of moles of each element.
1. Calculate the number of moles of platinum:
- Mass of platinum = 0.509 g
- The molar mass of platinum is 195.078 g/mol.
- Moles of platinum = mass of platinum / molar mass of platinum
= 0.509 g / 195.078 g/mol
2. Calculate the number of moles of chlorine:
- Mass of chlorine = The total mass of the compound - mass of platinum
= 0.889 g - 0.509 g
- The molar mass of chlorine is 35.453 g/mol.
- Moles of chlorine = mass of chlorine / molar mass of chlorine
3. Determine the empirical formula using the mole ratios:
- Divide the moles of each element by the smallest number of moles obtained.
- Round the ratios to the nearest whole number.
Now, let's plug in the values and calculate the empirical formula.
To find out the empirical formula of the compound formed by the reaction of pure platinum metal with HCl, we need to determine the ratio of platinum to chlorine atoms in the compound.
1. Calculate the mass of platinum in the compound:
Mass of platinum = Mass of the compound - Mass of chlorine
Mass of platinum = 0.889 g - (Mass of chlorine)
2. Determine the number of moles of platinum:
Moles of platinum = Mass of platinum / Molar mass of platinum
3. Determine the number of moles of chlorine:
Moles of chlorine = Mass of chlorine / Molar mass of chlorine
4. Find the mole ratio of platinum to chlorine:
Divide the moles of platinum and chlorine by the smallest number of moles. Round to the nearest whole number to get the ratio. This ratio will represent the subscripts in the empirical formula.
For a more accurate calculation, we need to know the molar mass of platinum. The molar mass of platinum is approximately 195.1 g/mol. The molar mass of chlorine is approximately 35.45 g/mol.