Final answer:
To find out how much cadmium sulfide could be produced from 22.0 g of cadmium metal, a stoichiometric calculation is performed, assuming a 1:1 ratio between cadmium and sulfur based on the provided data and the molar mass of cadmium. The calculation implies that 22.0 g of cadmium would theoretically yield 22.0 g of cadmium sulfide, given an excess of sulfur and 100% yield.
Step-by-step explanation:
The student's question pertains to solving a stoichiometry problem involving the reaction of cadmium metal with sulfur to produce cadmium sulfide (CdS). In order to determine how much cadmium sulfide can be produced from 22.0 g of cadmium metal, we first need to use the information provided that 112.4 g of cadmium reacts with 32.1 g of sulfur to calculate the stoichiometric ratio. Here, no specific reaction equation is provided, but we assume it's Cd + S → CdS based on the materials given and the common valencies of cadmium and sulfur.
From the initial information, we can determine the molar mass of cadmium (112.4 g/mol) and use it to calculate the moles of cadmium involved in the initial reaction. However, because we have the masses of both the cadmium and sulfur, this problem becomes simpler, assuming a 1:1 mole ratio since the reaction appears to be between one atom of cadmium and one atom of sulfur. This assumption leads to:
- The amount of cadmium sulfide produced is directly proportional to the amount of cadmium reacting, given a constant excess of sulfur.
Therefore, we can set up a proportion:
(112.4 g Cd / 32.1 g S) = (22.0 g Cd / x g S)
From this proportion, we calculate the amount of sulfur that would react with 22.0 g of cadmium. However, since we do not need this to find the final mass of cadmium sulfide, we use the stoichiometry of the reaction, which suggests for each gram of Cd, one gram of CdS is formed (assuming 100% yield and atomic weight of sulfur is much lower and thus doesn't significantly affect the mass). Hence, 22.0 g of Cd would theoretically yield 22.0 g of CdS.