use the following equation, which represents a reaction used commercially to produce elemental arsenic by heating arsenic (III) oxide with carbon. 2AS2O3 +3C ---->3CO2 + 4As If 6.0 mol of each reactant are available for the above reaction, the mixture remaining after the reaction should contain a. 4.0 mol As2O3
use the following equation, which represents a reaction used commercially to produce elemental arsenic by heating arsenic (III) oxide with carbon.
2AS2O3 +3C ---->3CO2 + 4As
If 6.0 mol of each reactant are available for the above reaction, the mixture remaining after the reaction should contain
a. 4.0 mol As2O3
b. 3.0 mol C.
c 2.0 mol As2O3
d. no reactants.
If 6.0 mol of each reactant are available for the above reaction, the mixture remaining after the reaction should contain
a. 4.0 mol As.
b. 4.0 mol CO2
c. 6.0 mol CO2
d. equal quantities of the products.
If 8.0 mol As2O3 reacts with excess carbon, the theoretical yield of the above reaction is
a. 32 mol As.
b. 16 mol As
c. 8 mol As.
d. 4 mol As.
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In step 2 , why do we need to find the limiting reactant first?
In step 3 , why did we subtract 6 mol with 4 mol?
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