In an experiment, 6.700g of hydrogen sulfide is fully decomposed into its elements.If 0.396g of hydrogen is obtained in this experiment, how many grams of sulfur must be obtained?
H2S ==> H2 + S
mols H2S = grams/molar mass
mols H2 = mols H2S (from the coefficients).
g H2 = mols x molar mass. This is the theoretical yield.
% yield = (0.396/theor yield)*100 = ?
Then mols H2S x molar mass S x (theor yield/100) = g S.
4.5?
To determine the amount of sulfur obtained, we need to use the law of conservation of mass, which states that in a chemical reaction, the mass of the reactants is equal to the mass of the products.
First, we need to find the mass of hydrogen sulfide that decomposed. We are given that 0.396g of hydrogen was obtained from the reaction. Since the molar ratio of hydrogen to hydrogen sulfide is 2:1, we can calculate the mass of hydrogen sulfide.
Step 1: Calculate the molar mass of hydrogen
The molar mass of hydrogen (H2) is 2 grams/mol because hydrogen has an atomic mass of 1 g/mol, and there are 2 hydrogen atoms in each molecule of H2.
Step 2: Convert the mass of hydrogen to moles
To convert grams to moles, we can divide the mass of hydrogen by its molar mass:
0.396 g / (2 g/mol) = 0.198 mol of hydrogen
Step 3: Calculate the mass of hydrogen sulfide
Using the molar ratio of hydrogen to hydrogen sulfide (2:1), we can determine the moles of hydrogen sulfide:
0.198 mol of hydrogen * (1 mol of H2S / 2 mol of H2) = 0.099 mol of H2S
Finally, since the molar mass of hydrogen sulfide (H2S) is 34 grams/mol (1 mol of H2 + 32 g/mol of S), we can calculate the mass of sulfur:
Step 4: Calculate the mass of sulfur
0.099 mol of H2S * (32 g/mol of S) = 3.168 g of sulfur
Therefore, approximately 3.168 grams of sulfur must be obtained in this experiment.