What Is the Average Atomic Mass of M in M2S3?

AI Thread Summary
To determine the average atomic mass of M in M2S3, a 4.000g sample loses 0.277g upon heating, resulting in a mass of 3.733g for MO2. The balanced reaction equation is M2S3 + O2 -> MO2 + SO2, which allows for the calculation of the molar mass of M. The discussion highlights the need to express the mass of MO2 in terms of the masses and molar masses of the reactants. Clarification is sought on the calculation of the MO2 mass, indicating potential confusion in the initial assessment. The key to solving the problem lies in correctly balancing the reaction and applying stoichiometric relationships.
George3
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Homework Statement


When M2S3 is heated in air, it is converted to MO2. A 4.000g sample of M2S3 shows a decrease in mass of .277 g when it is heated in air. What is the average atomic mass of M?


Homework Equations





The Attempt at a Solution


I don't not really know how to tackle this problem. I know the mass of MO2 would be 3.833g.
 
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Your problem description indicates that 0.277 grams of M2S3 gave its stoichiometric amount of MO2. How do you know that the mass of MO2 is 3.833 grams as you say in your solution attempt? Your description does not give enough information for that. I might be missing something in my logic.
 
I think George means 3.733.

George, start with a balanced reaction equation:

M2S3 + O2 -> MO2 + SO2

Try to express mass of MO2 produced in terms of masses and molar masses or reagents, that should give you one equation with one unknown - molar mass of M.
 
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