Answer:
Maximum mass of Water that could be produced = 4.34 g
Explanation:
Balanced equation for this reaction:
As we can see from the balanced equation 1 mol of ethane reacts with 7/2 mol of oxygen to give 2 mol of carbon dioxide and 3 nol of water.
Now, from the given data in the question let's calculate the moles of ethane and oxygen.
Formula for calculate moles is,
Number of moles = Mass(in g) ÷ Molecular weight(in g/mol)
Moles of Ethane:
Mass of Ethane = 2.41 g
Molecular weight of Ethane = 30 g/mol
No. Of moles of Ethane = 2.41 g ÷ 30 g/mol
No. Of moles of Ethane = 0.0803 mol
Moles of Oxygen:
Mass of Oxygen = 18 g
Molecular weight of Oxygen (O2) = 32 g/mol
No. Of moles of Oxygen = 18 g ÷ 32 g/mol
No. Of moles of Oxygen = 0.5625 mol
Now, according to the balanced equation,
1 mol of Ethane reacts with 7/2 mol of Oxygen to give 3 mol of water.
So,
"0.0803 mol of Ethane" will react with,
"{0.0803×(7/2)} = 0.2811 mol of Oxygen" to give,
"0.0803×3 = 0.2409 mol of Water"
*Note that 0.0803 mol of ethane reacts with 0.2811 mol of Oxygen only. The rest of the moles of Oxygen i.e (0.5625-0.2811)=0.2814 mol of Oxygen remains unreacted.
So, now we found out that "2.41 g of Ethane = 0.0803 mol of Ethane" gives 0.2409 mol of Water.
So, now we need to convert moles of water into grams of water to get our answer.
We will use the following formula,
Mass(in g) = Moles × Molecular weight(in g/mol)
Moles of Water = 0.2409 mol
Molecular weight of Water = 18 g/mol
Put these values in the above formula for mass,
Mass of Water = 0.2409 mol × 18 g/mol
Mass of water = 4.3362 g
Rounding the answer to 3 significant digits give,
Mass of water = 4.34 g
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