hydrogen sulfide may be prepared in the laboratory by the action of hydrochloric acid on iron (2) sulfide. How much iron (2) sulfide would be needed to prepare 15L of hydrogen sulfide?
1. Write the equation and balance it.
2. Convert 15 L H2S to mols. Remember that 1 mol of a gas at STP will occupy 22.4 L.
3. Using the coefficients in the balanced equation, convert moles H2S to moles iron.
4. Convert moles iron to grams remembering that g = moles x molar mass.
By the way, if you want to write ferrous sulfide using the Stock system (now callled the IUPAC system), you should use Roman numerals as in iron(II) sulfide.
To determine the amount of iron(II) sulfide needed to prepare 15L of hydrogen sulfide, we need to use stoichiometry, which relates the amount of reactants and products in a chemical reaction.
The balanced chemical equation for the reaction between hydrochloric acid (HCl) and iron(II) sulfide (FeS) to form hydrogen sulfide (H2S) is:
FeS(s) + 2HCl(aq) → FeCl2(aq) + H2S(g)
From the equation, we can see that 1 mole of FeS reacts with 2 moles of HCl to produce 1 mole of H2S. We can use this information to determine the amount of FeS needed.
Step 1: Determine the molar volume of hydrogen sulfide:
The ideal gas law states that 1 mole of any gas occupies 22.4 liters at standard temperature and pressure (STP). Therefore, 1 mole of H2S occupies 22.4 liters at STP.
Step 2: Convert liters of H2S to moles of H2S:
Given that we want to produce 15 liters of H2S, we divide 15 by the molar volume of H2S (22.4 liters/mole) to find the number of moles:
15 liters H2S × (1 mole H2S / 22.4 liters H2S) = 0.67 moles H2S
Step 3: Use stoichiometry to determine moles of FeS:
From the balanced chemical equation, we know that 1 mole of FeS reacts with 1 mole of H2S. Therefore, the moles of FeS needed is equal to the moles of H2S:
0.67 moles H2S = 0.67 moles FeS
Step 4: Convert moles of FeS to grams of FeS:
The molar mass of FeS is 87.91 g/mol. Therefore, we can calculate the mass of FeS needed using its molar mass and the number of moles:
0.67 moles FeS × 87.91 g FeS/mol = 58.9 grams FeS
Therefore, approximately 58.9 grams of iron(II) sulfide would be needed to prepare 15L of hydrogen sulfide.
To determine the amount of iron(II) sulfide needed to prepare 15 liters of hydrogen sulfide, we need to consider the balanced chemical equation for the reaction between hydrochloric acid and iron(II) sulfide.
The balanced equation for this reaction is:
FeS + 2HCl -> H2S + FeCl2
From the balanced equation, we can see that 1 mole of iron(II) sulfide (FeS) reacts with 2 moles of hydrochloric acid (HCl) to produce 1 mole of hydrogen sulfide (H2S).
To find the amount of iron(II) sulfide needed, we can use the following steps:
1. Convert the given volume of hydrogen sulfide to moles using the ideal gas law. The ideal gas law equation is PV = nRT, where:
- P is the pressure of the gas
- V is the volume of the gas (in liters)
- n is the number of moles of gas
- R is the ideal gas constant (0.0821 L*atm/mol*K)
- T is the temperature in Kelvin
2. Simplify the stoichiometry by comparing the mole ratio between hydrogen sulfide and iron(II) sulfide. According to the balanced equation, we know that 1 mole of FeS reacts to produce 1 mole of H2S. Therefore, the moles of FeS needed will be the same as the moles of H2S.
3. Calculate the amount of iron(II) sulfide needed using the molar mass of FeS, which is 87.91 g/mol.
Now let's calculate the amount of iron(II) sulfide needed step by step:
Step 1: Convert the volume of hydrogen sulfide to moles
We are given the volume of hydrogen sulfide, which is 15 liters. However, it is important to know the temperature and pressure at which this volume of gas is measured to make accurate calculations. Please provide the temperature and pressure at which the gas volume is measured.
Step 2: Simplify the stoichiometry
As mentioned earlier, the stoichiometry of the balanced equation tells us that the moles of FeS needed will be the same as the moles of H2S. Since we have calculated the moles of H2S in Step 1, we can directly use that value.
Step 3: Calculate the amount of iron(II) sulfide needed
Multiply the moles of iron(II) sulfide (which is the same as the moles of hydrogen sulfide calculated in Step 1) by the molar mass of FeS (87.91 g/mol) to find the grams of iron(II) sulfide needed.
Note: It is important to handle and work with chemicals safely in a laboratory setting. Ensure you are following proper safety guidelines and procedures when handling hydrochloric acid and iron(II) sulfide, including wearing appropriate personal protective equipment (PPE) and conducting the experiment in a well-ventilated area.