Help!!!!!!!!!!!!
Fe + CuSO4 --> Cu + FeSO4
2.05g 7.00g 2.46g 151.8g
Which reactant was limiting and how does this chemical equation support this? The numbers beneath the names are the masses in grams.
PLease Help me!!!!!!!!!!!
The only thing this problem tells me is that the numbers don't add up. 9.05 g on the left does not equal 154.26
To determine which reactant is limiting, we need to calculate the moles of each reactant and compare them based on the stoichiometry of the balanced equation.
Let's start with the iron (Fe) reactant:
1. Calculate the moles of Fe:
moles of Fe = mass of Fe / molar mass of Fe
The molar mass of Fe (iron) is 55.845 g/mol.
moles of Fe = 2.05 g / 55.845 g/mol
moles of Fe = 0.0367 mol
Next, let's calculate the moles of copper sulfate (CuSO4):
1. Calculate the moles of CuSO4:
moles of CuSO4 = mass of CuSO4 / molar mass of CuSO4
The molar mass of CuSO4 is 159.609 g/mol.
moles of CuSO4 = 7.00 g / 159.609 g/mol
moles of CuSO4 = 0.0439 mol
According to the balanced equation, the stoichiometry implies a 1:1 ratio between Fe and CuSO4. This means that for every 1 mole of Fe, we need 1 mole of CuSO4.
Now, let's compare the moles of Fe and CuSO4. The ratio is:
moles of Fe : moles of CuSO4 = 0.0367 : 0.0439
Since the ratio is less than 1, this indicates that there is an excess of moles of CuSO4 compared to Fe. Therefore, Fe is the limiting reactant.
This chemical equation supports the conclusion that Fe is the limiting reactant because the calculated moles of Fe are less than the moles of CuSO4. The stoichiometry of the balanced equation confirms that Fe has the fewer moles required for the reaction to proceed, making it the limiting reactant.