Given the balanced equation, calculate the mass of product that can be prepared from 1.10 g of zinc metal.
2Zn(s)+O2(g)→2ZnO(s)
How to solve? Thanks.
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To solve this problem, you need to use stoichiometry, which is a way to relate the amount of one substance in a balanced chemical equation to the amount of another substance in the same equation.
Here's how you can solve the problem step by step:
Step 1: Write down the balanced equation:
2 Zn(s) + O2(g) → 2 ZnO(s)
Step 2: Calculate the molar mass of zinc:
The molar mass of zinc (Zn) can be found on the periodic table, and it is approximately 65.38 g/mol.
Step 3: Convert the mass of zinc to moles:
To convert grams of zinc (given in the problem) to moles, use the equation:
moles = given mass / molar mass of zinc
moles of zinc = 1.10 g / 65.38 g/mol
moles of zinc = 0.0168 mol
Step 4: Use the stoichiometry of the balanced equation:
According to the balanced equation, 2 moles of zinc react with 1 mole of oxygen (O2) to produce 2 moles of zinc oxide (ZnO).
Based on the stoichiometry, we can establish a ratio:
2 mol Zn : 2 mol ZnO
Step 5: Calculate the moles of zinc oxide produced:
To calculate the moles of zinc oxide produced, use the ratio from step 4:
moles of ZnO = moles of Zn * (2 mol ZnO / 2 mol Zn)
moles of ZnO = 0.0168 mol * (2/2)
moles of ZnO = 0.0168 mol
Step 6: Convert moles of zinc oxide to grams:
To convert moles of zinc oxide to grams, use the molar mass of zinc oxide (ZnO). The molar mass of ZnO is approximately 81.38 g/mol.
mass of ZnO = moles of ZnO * molar mass of ZnO
mass of ZnO = 0.0168 mol * 81.38 g/mol
mass of ZnO = 1.37 grams
Therefore, the mass of zinc oxide (ZnO) that can be produced from 1.10 grams of zinc (Zn) is approximately 1.37 grams.