im a little confuse on this problem.
"in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it]
A. If 100 g of CuS and 56 g of O2 are available, which reactant is limiting?
B. Which reactant is in excess, and how many grams remain after the reaction is completed?
if you could tell me how you do it would be realllly helpful as well.
Thank you!
To determine which reactant is limiting and which reactant is in excess in the given chemical reaction, we need to compare the stoichiometry of the reaction with the amounts of reactants given.
A. To determine which reactant is limiting, we need to calculate the moles of each reactant and compare their ratios.
1. Calculate the moles of CuS:
Molar mass of CuS = atomic mass of Cu + atomic mass of S = 63.55 g/mol + 32.07 g/mol = 95.62 g/mol
Moles of CuS = mass of CuS / molar mass of CuS = 100 g / 95.62 g/mol = 1.046 mol
2. Calculate the moles of O2:
Molar mass of O2 = 16.00 g/mol + 16.00 g/mol = 32.00 g/mol
Moles of O2 = mass of O2 / molar mass of O2 = 56 g / 32.00 g/mol = 1.75 mol
From the balanced equation, we can see that the mole ratio of CuS to O2 is 2:2, or 1:1. Therefore, we have equal moles of CuS and O2.
Since the number of moles is the same for both reactants, neither reactant is limiting. They are present in stoichiometric amounts.
B. Since neither reactant is limiting, none of them is in excess. Therefore, no reactant remains after the reaction is completed.
In summary:
A. Neither reactant is limiting.
B. Neither reactant is in excess, and no reactant remains after the reaction is completed.
Note: In case one reactant is in excess, you would need to calculate how much of the excess reactant remains using the stoichiometry of the balanced equation and the amount of the limiting reactant consumed.