An 8.00-gram sampleyields 1.64grams of Zinc when the compound is decomposed. What is the compound?
Are you positive you posted ALL of the information? I can conclude from the data this much but that's all.
ZnX ==> Zn + X
8.00 => 1.64 + 6.36
%Zn = *1.64/8.00)*100 = 20.5%
So %X = 79.5%
but I have no idea at all what X is.
To determine the compound, we need to understand the concept of compound stoichiometry and perform some calculations.
First, let's find the mass of oxygen in the compound. We have the mass of the sample (8.00 grams) and the mass of zinc obtained (1.64 grams). To find the mass of oxygen, we need to subtract the mass of zinc from the mass of the sample.
Mass of Oxygen = Mass of Sample - Mass of Zinc
Mass of Oxygen = 8.00 grams - 1.64 grams
Mass of Oxygen = 6.36 grams
Next, let's calculate the number of moles of zinc and oxygen in the compound. We can use the atomic masses of zinc and oxygen to convert their masses into moles.
Molar mass of Zinc (Zn) = 65.38 g/mol
Number of moles of Zinc = Mass of Zinc / Molar mass of Zinc
Number of moles of Zinc = 1.64 grams / 65.38 g/mol
Number of moles of Zinc ≈ 0.025 moles
Molar mass of Oxygen (O) = 16.00 g/mol
Number of moles of Oxygen = Mass of Oxygen / Molar mass of Oxygen
Number of moles of Oxygen = 6.36 grams / 16.00 g/mol
Number of moles of Oxygen ≈ 0.3975 moles
Now, let's find the ratio of moles between zinc and oxygen in the compound. We can divide the number of moles of zinc and oxygen by their smaller value to find the ratio.
Zinc to Oxygen ratio = Number of moles of Zinc / Number of moles of Oxygen
Zinc to Oxygen ratio ≈ 0.025 moles / 0.3975 moles
Zinc to Oxygen ratio ≈ 0.063
The ratio of zinc to oxygen is approximately 0.063.
Based on this ratio, we can determine the compound. The closest whole-number ratio of zinc to oxygen is 1:2. Therefore, the compound in question is most likely Zinc Oxide (ZnO).