Answer:
The answer to your question is Pd₂H₄
Explanation:
Data
mass of palladium = 42.56 g
mass of hydrogen = 0.8 g
Process
1.- Convert the grams of each substance to moles
106 g of Pd ----------------- 1 mol
42.56 g of Pd ------------- x
x = (42.56 x 1)/106
x = 0.402 moles
1 g of H --------------------- 1 mol
0.8 g of H ------------------ x
x = (0.8 x 1)/1
x = 0.8 moles
2.- Divide by the lowest number of moles
Palladium = 0.402/0.402 = 1
Hydrogen = 0.8/0.402 = 1.99 ≈ 2
3.- Write the empirical formula
PdH₂
4.- Calculate the mass of the empirical formula
PdH₂ = 106 + 2 = 108
5.- Divide the molar mass by the molar mass of the empirical formula
216.8/108 = 2
6.- Get the molecular formula
2(PdH₂) = Pd₂H₄
The molecular formula of the compound containing 42.56 g of palladium and 0.80 g of hydrogen is Pd₂H₄
We'll begin by calculating the empirical formula of the compound. This can be obtained as follow
Polladium (Pd) = 42.56 g
Hydrogen (H) = 0.80 g
Divide by their molar mass
Pd = 42.56 / 106.42 = 0.4
Hydrogen (H) = 0.80 / 1 = 0.8
Divide by the smallest
Pd = 0.4 / 0.4 = 1
H = 0.8 / 0.4 = 2
Thus, the empirical formula of the compound is PdH₂
Empirical formula => PdH₂
Molar mass of compound = 216.8 g/mol.
Molecular formula = Empirical formula × n = molar mass
[PdH₂]n = 216.8
[106.42 + (1×2)]n = 216.8
108.42n = 216.8
Divide both side by 108.42
n = 216.8 / 108.42
Molecular formula => [PdH₂]n
Molecular formula => [PdH₂]₂
Therefore, the molecular formula of the compound is Pd₂H₄
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