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1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excess
and how much ?
(At. wt. Mg = 24; O = 16)
and how much ?
(At. wt. Mg = 24; O = 16)
- a)Mg, 0.44 g
- b)O2, 0.28 g
- c)Mg, 0.16 g
- d)O2, 0.16 g
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which r...
Given: Mass of magnesium (Mg) = 1.0 g
Mass of oxygen (O2) = 0.56 g
Atomic weight of Mg = 24
Atomic weight of O = 16
To find out which reactant is left in excess, we need to first calculate the amount of each reactant required for the reaction using stoichiometry.
The balanced chemical equation for the reaction is:
2Mg + O2 → 2MgO
From the equation, we can see that 2 moles of Mg react with 1 mole of O2 to produce 2 moles of MgO.
Calculating the amount of Mg and O2 used in the reaction:
Moles of Mg = Mass of Mg / Atomic weight of Mg
Moles of Mg = 1.0 g / 24 g/mol
Moles of Mg = 0.0417 mol
Moles of O2 = Mass of O2 / Atomic weight of O2
Moles of O2 = 0.56 g / 32 g/mol
Moles of O2 = 0.0175 mol
From the balanced chemical equation, we can see that 1 mole of O2 is required to react with 2 moles of Mg. Therefore, the amount of O2 required to react with 0.0417 mol of Mg is:
Moles of O2 required = 0.0417 mol / 2
Moles of O2 required = 0.0209 mol
Comparing the amount of O2 required (0.0209 mol) with the amount of O2 available (0.0175 mol), we can see that O2 is the limiting reactant. This means that Mg is left in excess.
Calculating the amount of Mg left in excess:
Moles of Mg left = Moles of Mg used in the reaction - Moles of Mg required for the reaction
Moles of Mg left = 0.0417 mol - 0.0209 mol
Moles of Mg left = 0.0208 mol
Mass of Mg left = Moles of Mg left x Atomic weight of Mg
Mass of Mg left = 0.0208 mol x 24 g/mol
Mass of Mg left = 0.4992 g
Therefore, the reactant left in excess is Mg and the amount left is 0.16 g (rounded to two decimal places).
Mass of oxygen (O2) = 0.56 g
Atomic weight of Mg = 24
Atomic weight of O = 16
To find out which reactant is left in excess, we need to first calculate the amount of each reactant required for the reaction using stoichiometry.
The balanced chemical equation for the reaction is:
2Mg + O2 → 2MgO
From the equation, we can see that 2 moles of Mg react with 1 mole of O2 to produce 2 moles of MgO.
Calculating the amount of Mg and O2 used in the reaction:
Moles of Mg = Mass of Mg / Atomic weight of Mg
Moles of Mg = 1.0 g / 24 g/mol
Moles of Mg = 0.0417 mol
Moles of O2 = Mass of O2 / Atomic weight of O2
Moles of O2 = 0.56 g / 32 g/mol
Moles of O2 = 0.0175 mol
From the balanced chemical equation, we can see that 1 mole of O2 is required to react with 2 moles of Mg. Therefore, the amount of O2 required to react with 0.0417 mol of Mg is:
Moles of O2 required = 0.0417 mol / 2
Moles of O2 required = 0.0209 mol
Comparing the amount of O2 required (0.0209 mol) with the amount of O2 available (0.0175 mol), we can see that O2 is the limiting reactant. This means that Mg is left in excess.
Calculating the amount of Mg left in excess:
Moles of Mg left = Moles of Mg used in the reaction - Moles of Mg required for the reaction
Moles of Mg left = 0.0417 mol - 0.0209 mol
Moles of Mg left = 0.0208 mol
Mass of Mg left = Moles of Mg left x Atomic weight of Mg
Mass of Mg left = 0.0208 mol x 24 g/mol
Mass of Mg left = 0.4992 g
Therefore, the reactant left in excess is Mg and the amount left is 0.16 g (rounded to two decimal places).
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Community Answer
1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which r...
According to stoichiometry, 48g Mg is required to react with 32g of oxygen.
1g Mg needs 0.66g oxygen.
Hence, O is the limiting reagent.
0.56g oxygen requires 0.84g of Magnesium.
Since we took 1g Mg, 0.16g Mg remains in excess.
1g Mg needs 0.66g oxygen.
Hence, O is the limiting reagent.
0.56g oxygen requires 0.84g of Magnesium.
Since we took 1g Mg, 0.16g Mg remains in excess.
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1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excessand how much ?(At. wt. Mg = 24; O = 16)a)Mg, 0.44 gb)O2, 0.28 gc)Mg, 0.16 gd)O2, 0.16 gCorrect answer is option 'C'. Can you explain this answer?
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1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excessand how much ?(At. wt. Mg = 24; O = 16)a)Mg, 0.44 gb)O2, 0.28 gc)Mg, 0.16 gd)O2, 0.16 gCorrect answer is option 'C'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excessand how much ?(At. wt. Mg = 24; O = 16)a)Mg, 0.44 gb)O2, 0.28 gc)Mg, 0.16 gd)O2, 0.16 gCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excessand how much ?(At. wt. Mg = 24; O = 16)a)Mg, 0.44 gb)O2, 0.28 gc)Mg, 0.16 gd)O2, 0.16 gCorrect answer is option 'C'. Can you explain this answer?.
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