Fe(s) + Cu^2+(aq)--> Fe^2+(aq) +Cu(s)(1)
2Fe(s) + 3Cu^2+(aq)--> 2Fe^3+(aq) +3Cu(s) (2)
suppose that you use 1.110 g of Iron in this experiment what is the minimum volume of 1.0M of copper sulfate solution that you should add?
Hint: since you don't know wheteher equation 1 or 2 is the appropriat one you must base your calculations on whichever of tthe equations would require the most copper sulfate for any given quantity of iron?
lol..I tried and subsequently realised I didn't know what I was doing. any help would be appreciated
No. An equation is balanced only if mass is balanced AND charge is balanced. EQuation (2) balances both.
Check the charge changes to verify.
but she was looking for a numerical answer...are you saying the equation is flawed?
To determine the minimum volume of 1.0M copper sulfate solution needed, we need to compare the stoichiometry of equations 1 and 2.
Let's start by calculating the molar mass of iron (Fe):
Molar mass of Fe = Atomic mass of Fe = 55.845 g/mol
Next, let's calculate the number of moles of iron (Fe) used in the experiment:
Number of moles of Fe = Mass of Fe / Molar mass of Fe
Given that the mass of Fe used is 1.110 g, we can substitute this into the equation:
Number of moles of Fe = 1.110 g / 55.845 g/mol = 0.01987 mol
Now, we'll analyze equations 1 and 2 to determine how many moles of copper sulfate (CuSO4) are required for the given quantity of iron (Fe).
In equation 1, the stoichiometric ratio between iron (Fe) and copper sulfate (CuSO4) is 1:1. This means that for every 1 mole of Fe, we need 1 mole of CuSO4.
In equation 2, the stoichiometric ratio between iron (Fe) and copper sulfate (CuSO4) is 2:3. This means that for every 2 moles of Fe, we need 3 moles of CuSO4.
To determine which equation requires more copper sulfate (CuSO4) for the given quantity of iron (Fe), we compare the stoichiometric ratios. Equation 2 requires more moles of CuSO4 (3 moles) for 2 moles of Fe, while equation 1 requires only 1 mole of CuSO4 for 1 mole of Fe.
Since we want to base our calculations on the equation that requires the most copper sulfate (CuSO4), we will use equation 2.
In equation 2, we need 3 moles of CuSO4 for 2 moles of Fe. Therefore, the ratio of CuSO4 to Fe is 3:2.
Number of moles of CuSO4 = (Number of moles of Fe) * (3/2)
Number of moles of CuSO4 = 0.01987 mol * (3/2) = 0.02981 mol
Now, let's calculate the minimum volume of 1.0M copper sulfate (CuSO4) solution needed:
Molarity = Moles / Volume
Given that the molarity (M) is 1.0M and the number of moles of CuSO4 is 0.02981 mol, we can substitute these values into the equation:
1.0M = 0.02981 mol / Volume
Volume = 0.02981 mol / 1.0M = 0.02981 L = 29.81 mL
Therefore, the minimum volume of 1.0M copper sulfate (CuSO4) solution that should be added is 29.81 mL.