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)
IS THIS CORRECT?
Answered above.
Yes, your calculation is correct.
To calculate the mass of oxygen gas produced in the decomposition of 5.55 g of silver oxide, you need to use the balanced chemical equation and convert the given mass to moles, and then to the desired mass of oxygen gas.
Here's a step-by-step breakdown of your calculation:
1. Write the balanced chemical equation:
2 Ag2 O decomposes → 4 Ag + O2
2. Determine the molar mass of Ag2O:
Ag2O = 2(Ag) + 1(O) = 2(107.87 g/mol) + 16.00 g/mol = 139.868 g/mol
3. Set up the conversion factors to convert grams of Ag2O to moles of Ag2O:
5.55 g Ag2O * (1 mol Ag2O / 139.868 g Ag2O) = 0.0397 mol Ag2O
4. Use the stoichiometry of the balanced equation to find the number of moles of O2:
0.0397 mol Ag2O * (1 mol O2 / 1 mol Ag2O) = 0.0397 mol O2
5. Convert moles of O2 to grams of O2 using the molar mass of O2:
0.0397 mol O2 * (31.998 g O2 / 1 mol O2) = 1.27 g O2
Therefore, the mass of oxygen gas produced in the decomposition of 5.55 g of silver oxide is 1.27 g O2.
If you have more questions or need help with other problems, feel free to ask!