What mass of aluminum hydroxide will be produced when 0.460 grams of aluminum sulfide react with water? How many grams of hydrogen sulfide are produced, according to the following equaton?
Al2S3 + H20 -------> Al(OH)3 + H2S
First, balance the equation:
Al2S3 + 6H2O --> 2Al(OH)3 + 3H2S
Al2S3 = 150g/mol
H2S = 34g/mol
.46g of Al2S3 is 0.003 mole
each mole of Al2S3 produces 3 moles of H2S, so you'd get
.009moles of H2S = 0.313g
http://www.jiskha.com/science/chemistry/stoichiometry.html
To solve this problem, we can start by balancing the chemical equation:
Al2S3 + 6H2O → 2Al(OH)3 + 3H2S
Now, we can use stoichiometry to find the mass of aluminum hydroxide and hydrogen sulfide produced.
1. Calculating the mass of aluminum hydroxide (Al(OH)3)
To find the mass of aluminum hydroxide produced, we need to know the molar mass of Al(OH)3. Here are the molar masses of each element involved:
Aluminum (Al) = 26.98 g/mol
Oxygen (O) = 16.00 g/mol
Hydrogen (H) = 1.01 g/mol
To calculate the molar mass of Al(OH)3:
(1 * Al) + (3 * O) + (3 * H)
= (1 * 26.98) + (3 * 16.00) + (3 * 1.01)
= 26.98 + 48.00 + 3.03
= 77.01 g/mol
Next, we can use stoichiometry to convert the mass of Al2S3 to the mass of Al(OH)3.
0.460 g Al2S3 * (1 mol Al2S3 / 150.16 g Al2S3) * (2 mol Al(OH)3 / 1 mol Al2S3) * (77.01 g Al(OH)3 / 1 mol Al(OH)3)
The molar mass of Al2S3 is 150.16 g/mol.
0.460 * (2 * 77.01) / 150.16 = 0.4726 g
Therefore, approximately 0.473 grams of aluminum hydroxide will be produced.
2. Calculating the mass of hydrogen sulfide (H2S)
To find the mass of hydrogen sulfide produced, we can use the same stoichiometry approach.
0.460 g Al2S3 * (1 mol Al2S3 / 150.16 g Al2S3) * (3 mol H2S / 1 mol Al2S3) * (34.08 g H2S / 1 mol H2S)
0.460 * (3 * 34.08) / 150.16 = 0.293 g
Therefore, approximately 0.293 grams of hydrogen sulfide will be produced.
In summary:
- The mass of aluminum hydroxide produced is approximately 0.473 grams.
- The mass of hydrogen sulfide produced is approximately 0.293 grams.