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3.) Calculate the mass of oxygen gas that can be produced in the decomposition of 5.55 g of silver oxide.

This is what I did but is it right?... I need help with a few more btw to double check if i'm doing these right.

So here is what I did:
First: balance the equation
2 Ag2 O decomposes→ 4 Ag + O2

So, (btw I put parenthesis to make it visibly understandable if it helps)
5.55 g Ag2O * (1 mole Ag2O/ 139.868 g Ag2O) * (1 mol O2/ 1 mol Ag2O) * (31.998 g O2/ 1 mole O2) = 1.27 g O2.... since the ? is asking to calculate the mass of Oxygen gas (O2)

1.) what mass of zinc is needed to completely react with 4.00 g of silver nitrate?

2.) If excess ammonium sulfate reacts with 22.5 g of calcium hydroxide according to the following unbalanced chemical equation:
(NH4)2 SO4 + Ca (OH)2 → CaSO4 + NH3 + H2O

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1 answer
  1. I didn't check 2. #1 is not right but the system is correct.
    1. Your calculation for molar mass of Ag2O is not right. The molar mass is closer to 231.8. You obtained that number by 1Ag + 2O and it should be 2Ag + 1 O or (2*107.9)+ 16 = about 231.8.

    2. The second error is in convert mols Ag2O to mols O2. That should be
    mols Ag2O x (1 mol O2/2 mols Ag2O) = ?

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