Balanced Equation: 2Mg + O2 ---> 2MgO
Givens:
15.0 grams Mg
5.00 grams O2
Atomic Mass of O2- 32.0 grams
Atomic mass of Mg- 24.3 grams
Molecular mass- 40.3 MgO
Ratio- 2 moles : 1 mole : 2 mole
First you have to determine the limiting reactant by converting to moles:
15.0 g / (24.3 g) = .617 moles Mg
5.00 g / (32.0 g) = .156 moles O2
Because there is less of the oxygen, it is the limiting reactant and what the rest of the problem will be based on.
For the second part, you are given grams of oxygen and you are converting it to grams of magnesium oxide.
5.00 grams O2 / (32.0 grams O2)
first you get a balance equation 2Mg + O2 -> 2MgO
then you turn grams into moles
50g divide by the mass of Mg
so 50/24.32 = approx. 2.0567
now go from moles of magnesium to moles oxygen
2.0567 mol Mg * (1 mol O2 / 2 mol Mg) = approx. 1.0284 mol O2
but we want grams of Mg, so
1.0284mol O2 * (32g O2/ 1 mol O2) = approx. 32.9 g O2
The balanced equation of the reaction between Mg and O is:
2Mg + O2 --> 2MgO
The ratio of Mg to O2 is 2:1
Atomic mass of Mg : 24g/mol
2Mg = 2(24) = 48g/mol
Molecular mass of O2 : 2(16) = 32g/mol
Ratio of mass Mg to mass O2 = 48:32 = 3:2
Balanced Equation: 2Mg + O2 ---> 2MgO
Givens:
15.0 grams Mg
5.00 grams O2
Atomic mass of O2- 32.0 grams
Atomic mass of Mg- 24.3 grams
Molecular mass- 40.3 MgO
Ratio- 2 moles : 1 mole : 2 mole
First you have to determine the limiting reactant by converting to moles:
15.0 g / (24.3 g) = .617 moles Mg
5.00 g / (32.0 g) = .156 moles O2
Because there is less of the oxygen, it is the limiting reactant and what the rest of the problem will be based on.
For the second part, you are given grams of oxygen and you are converting it to grams of magnesium oxide.
5.00 grams O2 / (32.0 grams O2) × (2 moles MgO) × (40.3 grams MgO) = 12.6 grams MgO
well according to the Law of Conservation, what ever you start off with, u must end of with, no more, no less. so i would say that you would have 30g of aluminum oxide...
Unless there has been a MASSIVE loss of energy in the reaction (as in an explosion, very long burn, or absurdly bright light generation) it should be about 50g (35g + 15g).
ratio between oxygen usage to oxygen uptake is called as Oxygen extraction ratio
If 85.65g of iron forms 118.37g of the oxide, the mass of oxygen combined with this mass of iron is 32.72g. Calculate the number of moles of iron and oxygen which have combined (after all, the formula of a compound shows the ratio of the number of moles of each element combined). Do this by dividing the mass reacted by the Relative Atomic Mass of the element concerned. i.e. For Iron it is 85.65/55.8 and for Oxygen 32.72/16. This gives a mole ratio of Fe:O as 1.53:2.04 or 3:4 Therefore the formula is Fe3O4
No, the ratio of nitrogen to oxygen is not changed by altitude.
(2.5 grams =) 0.0393 moles of copper reacts with (0.31* grams =) 0.0194 moles of oxygen to produce something that has a ratio of 2.0 moles copper to 1 mole oxygen. Copper has a +1 and a +2 oxidation state and Oxygen has (usually) a -2 oxidation state so we know it isn't CuO because that's a 1:1 ratio. Cu2O has a 2:1 ratio...what could it be? *notice that the subtraction: 2.81g - 2.50 g = 0.31 g, reduced my significant digits to two.
When magnesium burns in air it creates a very bright white flame. When magnesium and oxygen mix,(mixing a substance with oxygen is called oxydation)it creates a new substance called magnesium oxide, which is a white powder. 2Mg+O2-----> 2MgO Magnesium oxide is a compound.
The formula is MgO, which represents a ratio of 1:1.
If the magnesium is not polished, there may be impurities or oxides on the surface that could affect the reported mole ratio of oxygen to magnesium. This could result in a higher reported mole ratio due to the presence of excess oxygen-containing compounds on the surface, leading to an inaccurate measurement of the actual ratio of oxygen to magnesium.
No. According to the law of definite proportions, the mole ratio will always be the same.
magnesium oxide is made up of two elements magnesium & oxygen..
Magnesium oxide (MgO) has one magnesium atom and one oxygen atom per molecule.
You will end up having less oxygen because it goes in doubles, and it is considered as flammable, and magnesium wouldn't burn if you didn't trap oxygen inside the magnesium foil. Some of the Magnesium WILL boil away as it burns, but you will end up with less oxidation anyway.
Magnesium : Iodine = 1:2
Balanced Formula:2Mg + O2 --> 2MgOMole ratio:2 : 1 : 2Givens:.486 g oxygen.738 g magnesium24.3 g = atomic mass of magnesium16.0 g = atomic mass of oxygen40.3 g = molecular mass of magnesium oxideFind the amount (in moles) of Magnesium oxide that oneelement will make:(.486 g O) / (16.0 g O) × (2 moles MgO)= .0608 moles MgO(.783 g Mg) / (24.3 g Mg) = .0322 moles MgOThere is less MgO produced with magnesium than oxygen; therefore, magnesium is the limiting reactant and the oxygen is the excess reactant. The magnesium determines how much Magnesium oxide is produced. It would be good to get .0608 moles of MgO, but there isn't enough magnesium. So the amount of MgO produced will be determined on the amount of Magnesium.Convert moles of MgO produced with the amount of oxygen to grams:.0322 mol MgO (40.3 g) = 1.30 grams of MgO produced--------------------------------------------------------------------------------------------------------You will need 3 moles of oxygen if you start with six moles of magnesium. This will allow you to produce 6 moles of magnesium oxide.Source: (e2020)
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The ratio of the total kinetic energies of eight grams of both oxygen and hydrogen at the same temperature is 1:2 respectively.
2Mg + O2 ---> 2MgO Magnesium burns in air forming magnesium oxide
ratio between oxygen usage to oxygen uptake is called as Oxygen extraction ratio