3.) One method used in the eighteen century to generate hydrogen was to pass steam through red-hot steel tubes. The following reaction takes place:
3Fe(s)+4H20(g)--->Fe3O4(s)+4H2(g)
2. What mass of iraon will react with 500.0 L of steam at 25 degrees C and 1.00 atm pressure?
3. If 285g of Fe3O4 are formed, what volume of hydrogen, measured at 20 degrees C and 1.06 atm, is produced?
I don't understand have to use which formula to plug in which numbers for number two in order to find the answers, or for number three.
3. has questions 2 and 3 included, so its really not one question, its one question with three parts, but i have one part answered i just don't understand these two.
You need to be more specific. I worked problem 3.) for you yesterday and included all the steps, including answers to each step. #2 is worked essentially the say way as is #3. We try very hard to help but help is all we do. You posted three questions and I worked one. I shall be happy to help you work 2 and 3 but I won't do them for you. You may be confused about which numbers to plug into which formulas. Go back over the problem I worked for you. I shall be happy to help you understand the problem I worked. If you understand the steps in that problem then it should be easier to work 2 and 3.
To solve these problems, you need to use the concept of stoichiometry, which relates the amounts of substances involved in a chemical reaction. In this case, you have the balanced equation:
3Fe(s) + 4H2O(g) ---> Fe3O4(s) + 4H2(g)
2. To find the mass of iron (Fe) that will react with 500.0 L of steam, you can follow these steps:
Step 1: Convert the given volume from liters to moles of water (H2O). To do this, you need to use the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Given:
Pressure (P) = 1.00 atm
Volume (V) = 500.0 L
Temperature (T) = 25°C = 298 K (converted to Kelvin)
Step 2: Calculate the number of moles of water.
n(H2O) = PV/RT
Substituting the given values:
n(H2O) = (1.00 atm) * (500.0 L) / (0.0821 L.atm/mol.K * 298 K)
Solve for n(H2O).
Step 3: Determine the molar ratio between Fe and H2O in the balanced equation. In this case, the ratio is 3 mol Fe : 4 mol H2O.
Step 4: Use the molar ratio to find the number of moles of Fe that will react.
n(Fe) = (n(H2O) * 3 mol Fe) / 4 mol H2O
Step 5: Convert moles of Fe to grams by using the molar mass of Fe, which is 55.85 g/mol.
mass(Fe) = n(Fe) * molar mass(Fe)
Substitute the calculated value of n(Fe) into the equation and solve for mass(Fe).
3. To find the volume of hydrogen (H2), you can follow similar steps:
Step 1: Convert the given mass of Fe3O4 to moles using its molar mass, which is 231.54 g/mol.
moles(Fe3O4) = mass(Fe3O4) / molar mass(Fe3O4)
Step 2: Determine the molar ratio between H2 and Fe3O4 in the balanced equation. In this case, the ratio is 4 mol H2 : 1 mol Fe3O4.
Step 3: Use the molar ratio to find the number of moles of H2 produced.
n(H2) = (moles(Fe3O4) * 4 mol H2) / 1 mol Fe3O4
Step 4: Convert moles of H2 to volume using the ideal gas law equation and the given conditions.
V(H2) = (n(H2) * R * T) / P
Given:
Pressure (P) = 1.06 atm
Temperature (T) = 20°C = 293 K (converted to Kelvin)
Substitute the calculated value of n(H2) into the equation and solve for V(H2).
These steps allow you to calculate the mass of iron that will react with the given volume of steam and the volume of hydrogen produced from a given mass of Fe3O4.