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The mass of CO2 produced from 620 gm mixture of C2H4O2 & O2, prepared to produce maximum energy is
- a)413.33 gm
- b)593.04 gm
- c)440 gm
- d)320 gm
Correct answer is option 'C'. Can you explain this answer?
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The mass of CO2produced from 620 gm mixture of C2H4O2& O2, prepare...
1) Let the mass of Acetic acid (C2H4O2) be x g, then mass of Oxygen gas O2 is (620-x) g.
Molecular Mass of Acetic acid (C2H4O2) = 60g
Molecular Mass of Oxygen Gas (O2) = 32g
2) To produce maximum energy, both reactants should be consumed fully.
To do that,
no. of moles of acetic acid / no. of moles of O2 = 1/2
=> n ( Acetic Acid) * 2 = n( Oxygen) * 1
Mass of acetic acid = x
Let mass of CO2 obtained be (m) gram.
3) Now by observing reaction,
1 / n(Acetic acid) = 2 / n(CO2)
=> n (Acetic acid) * 2 = n(CO2) * 1
Most Upvoted Answer
The mass of CO2produced from 620 gm mixture of C2H4O2& O2, prepare...
In order to determine the mass of CO2 produced from a mixture of C2H4O2, we need to first balance the chemical equation for the combustion of C2H4O2:
C2H4O2 + 3O2 → 2CO2 + 2H2O
From the balanced equation, we can see that for every 1 mole of C2H4O2 that is combusted, 2 moles of CO2 are produced. We can use this information to calculate the moles of C2H4O2 in the mixture:
moles of C2H4O2 = mass of C2H4O2 / molar mass of C2H4O2
= 620 g / 60 g/mol
= 10.33 moles
Since the stoichiometry of the balanced equation tells us that 1 mole of C2H4O2 produces 2 moles of CO2, we can calculate the moles of CO2 produced:
moles of CO2 = 2 × moles of C2H4O2
= 2 × 10.33
= 20.66 moles
Finally, we can convert the moles of CO2 to mass:
mass of CO2 = moles of CO2 × molar mass of CO2
= 20.66 × 44 g/mol
= 908.24 g
Therefore, the mass of CO2 produced from 620 g of C2H4O2 is approximately 908.24 g.
C2H4O2 + 3O2 → 2CO2 + 2H2O
From the balanced equation, we can see that for every 1 mole of C2H4O2 that is combusted, 2 moles of CO2 are produced. We can use this information to calculate the moles of C2H4O2 in the mixture:
moles of C2H4O2 = mass of C2H4O2 / molar mass of C2H4O2
= 620 g / 60 g/mol
= 10.33 moles
Since the stoichiometry of the balanced equation tells us that 1 mole of C2H4O2 produces 2 moles of CO2, we can calculate the moles of CO2 produced:
moles of CO2 = 2 × moles of C2H4O2
= 2 × 10.33
= 20.66 moles
Finally, we can convert the moles of CO2 to mass:
mass of CO2 = moles of CO2 × molar mass of CO2
= 20.66 × 44 g/mol
= 908.24 g
Therefore, the mass of CO2 produced from 620 g of C2H4O2 is approximately 908.24 g.
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