1g of Mg is burnt with 0.56 g O2 in a closed vessel. which reactant. is in excess and how much
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Burning of Magnesium:
2Mg + O2 → 2MgO
Mass of Mg = 1g
Molar Mass of Mg = 24g
Moles of Mg = 124= 0.041mol
Mass of O2 = 0.5g
Molar mass of O2 = 32g
Moles of O2 = 0.532 = 0.015mol
1mol of O2 reacts with 2 moles of Mg
Therefore, 0.015mol will react with 2×0.015mol of Mg i.e., 0.03mol of Mg.
Since we have 0.041mol of Mg, so (0.041-0.03)mol = 0.011mol of Mg will be left over and Oxygen will be limiting reagent.
Amount of MgO formed in the reaction:
1 mol of O2 gives 2 moles of MgO, so 0.015mol of O2 will give 0.03mol og MgO.
Molar mass of MgO = 40.3g
Mass of MgO formed = molar mass × moles = 40.3×0.03 = 1.209g
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2Mg + O2 → 2MgO
Mass of Mg = 1g
Molar Mass of Mg = 24g
Moles of Mg = 124= 0.041mol
Mass of O2 = 0.5g
Molar mass of O2 = 32g
Moles of O2 = 0.532 = 0.015mol
1mol of O2 reacts with 2 moles of Mg
Therefore, 0.015mol will react with 2×0.015mol of Mg i.e., 0.03mol of Mg.
Since we have 0.041mol of Mg, so (0.041-0.03)mol = 0.011mol of Mg will be left over and Oxygen will be limiting reagent.
Amount of MgO formed in the reaction:
1 mol of O2 gives 2 moles of MgO, so 0.015mol of O2 will give 0.03mol og MgO.
Molar mass of MgO = 40.3g
Mass of MgO formed = molar mass × moles = 40.3×0.03 = 1.209g
Mark it as brainly answer
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