60%
Mg+O2----->MgO
The balanced equation for the reaction between MgO and H2O is MgO + H2O -> Mg(OH)2.
Double bond Mg=O
Mg grams -> (use Mg's molar mass) -> Mg moles -> (use ratio of moles - use balanced equation) -> MgO moles -> (use MgO's molar mass) -> grams MgO set up the equation: Mg + O2 --> MgO (we know the product is MgO and not MgO2 because magnesium has a charge of 2+ while oxygen has a charge or 2-) balance the equation: 2Mg + O2 --> 2MgO Molar mass of Mg: 24.31 g/mol Molar mass of MgO: 44.30 g/mol (add the molar mass of Magnesium - 24.31g/mol and the molar mass of Oxygen - 15.99g/mol together) (use periodic table to find these) 7.0 grams of Mg To find the moles of Magnesium you use the molar mass of Mg. (7.0 g Mg)*(1 mol Mg / 24.31 g Mg) =0.2879 moles Mg notice how the grams cancel to leave you with moles - remember dividing by a fraction is the same as multiplying by the reciprocal Now use the balanced equation's coefficients and the moles of Mg to determine the number of moles of MgO present. 2Mg + O2 --> 2MgO 2 moles Mg : 2 moles MgO -> divide both sides by 2 and it obviously becomes a 'one to one' ratio. This means that the number of moles of Mg is equal to the number of moles of MgO. This means that there are 0.2879 moles of MgO. Now that we know MgO's molar mass and the number of moles of MgO we have, the grams of MgO produced can be determined. (0.2879 moles MgO)*(44.30 g MgO / 1 mol MgO) = 12.75 grams MgO
60%
60%
The percent of Mg calculated will be too high. Let's say that you reacted 1.00 g of Mg and made some MgO, but so much MgO escaped as smoke that only 1.00 g of MgO was left. You would then conclude from the numbers that the mass of O in the MgO was zero! This would lead you to conclude that the percent of Mg in the MgO was 100 %, which is silly and clearly in error. Although this is an extreme example, it illustrates that the loss of MgO as smoke from the crucible leads to a percent of Mg (calculated) that is above the expected 60.3 %.
2 Mg(OH)2 have 10 atoms.
Mg+O2----->MgO
"MgO" is magnesium oxide and "H" is hydrogen, as in "Mg + H(2)O => MgO + H(2)" MgO + H2 ---> H2O + Mg
They simply form Mg(OH)2
mgo+h2o=mg(OH)2 AAHana
The balanced equation for the reaction between MgO and H2O is MgO + H2O -> Mg(OH)2.
60%
MgOH(s)-----> MgO(s)+ H2O(g)
2Mg + O2 --> 2MgO First, take the amount given (2.033g Mg) and convert it to moles. 1 mole of Mg weighs 24.312g. Then, convert to the desired element, which is MgO. Then convert the moles of MgO into grams. The complete problem looks like this: 2.033g Mg(1 mol Mg/24.312g Mg)(2 mol MgO/2 mol Mg)(40.311g MgO/1 mol MgO) = 3.371 g MgO 3.371 g MgO should be produced.