provide with enough heat, magnesium and oxygen can undergo a synthesis reaction. how much magnesium is neede if 3.5kg of product is desired?
there is also part a) and b) to this qoustion that i wrote. i forgot to write it sorry.
a) what amount of oxygen is neede to react completely with 2.4g of magnesium?
b) if i have 2g of magnesium and 5g of oxygen, which reactant will run out first???
All of these are stoichiometry problems. See that example post.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the amount of magnesium needed for the synthesis reaction, we first need to know the balanced chemical equation for the reaction. The reaction between magnesium and oxygen is represented by:
2Mg + O2 â 2MgO
From the balanced equation, we can see that 2 moles of magnesium (Mg) are required to produce 2 moles of magnesium oxide (MgO). Now we need to find the molar mass of magnesium to convert the desired mass into moles.
The molar mass of magnesium (Mg) is approximately 24.31 g/mol. To convert the desired mass of 3.5 kg into grams, we multiply by 1000:
3.5 kg = 3500 g
Now, we can calculate the number of moles of magnesium needed using the molar mass:
Number of moles of Mg = Mass of Mg / Molar mass of Mg
Number of moles of Mg = 3500 g / 24.31 g/mol
Calculating this gives us:
Number of moles of Mg â 143.86 mol
However, remember that the balanced equation shows that 2 moles of magnesium are required to produce 2 moles of magnesium oxide. So, if you want to produce 3.5 kg of magnesium oxide, you need to double the moles of magnesium. Therefore:
Number of moles of Mg needed = 143.86 mol à 2 = 287.72 mol
So, approximately 287.72 moles of magnesium are needed to produce 3.5 kg of magnesium oxide.