If 48.1 g of solid Al2S3 and 6.68 mL of liquid H2O are reacted stoichiometrically according to the balanced equation, how many grams of solid Al2S3 remain?
Al2S3(s) + 6H2O(l) ¡æ 2Al(OH)3(s) + 3H2S(g)
Molar Mass (g/mol)
Al2S3 150.16
H2O 18.015
H2O 0.9982
Molar Volume (L)
22.4 at STP
Gas Constant
(L.atm.mol-1.K-1)
0.0821
To find out how many grams of solid Al2S3 remain after the reaction, we need to follow these steps:
1. Calculate the moles of Al2S3 and H2O used in the reaction:
- Given mass of Al2S3: 48.1 g
- Molar mass of Al2S3: 150.16 g/mol
- Moles of Al2S3 = mass / molar mass = 48.1 g / 150.16 g/mol
- Given volume of H2O: 6.68 mL
- Molar volume of H2O at STP: 22.4 L/mol
- Moles of H2O = volume / molar volume = 6.68 mL / 1000 mL/L / 22.4 L/mol
2. Determine the stoichiometric ratio between Al2S3 and Al(OH)3:
- According to the balanced equation, the stoichiometric ratio between Al2S3 and Al(OH)3 is 1:2.
3. Identify the limiting reactant:
- To determine the limiting reactant, compare the mole ratios of reactants using the stoichiometric ratio from the balanced equation.
- The reactant that is present in fewer moles is the limiting reactant.
- Let's calculate the mole ratio of Al2S3 and Al(OH)3:
Moles of Al(OH)3 = 2 * Moles of Al2S3
- Compare the moles of Al2S3 and Al(OH)3. If the mole ratio of Al2S3 to Al(OH)3 is greater than 1/2, then Al2S3 is the limiting reactant. Otherwise, H2O is the limiting reactant.
4. Calculate the moles of Al2S3 reacted:
- If Al2S3 is the limiting reactant, then the moles of Al2S3 reacted are equal to the initial moles of Al2S3.
5. Calculate the moles of Al(OH)3 formed:
- If Al2S3 is the limiting reactant, then the moles of Al(OH)3 formed are twice the moles of Al2S3 reacted.
6. Calculate the mass of Al2S3 remaining:
- The moles of Al2S3 remaining can be obtained by subtracting the moles of Al2S3 reacted from the total moles of Al2S3 initially.
- The mass of Al2S3 remaining is calculated by multiplying the moles of Al2S3 remaining by the molar mass of Al2S3.
Please provide the values for the molar mass of H2O, the molar volume of H2O at STP, and the gas constant to proceed with the calculation.