the number of moles of oxygen gas needed to react with 4.0 moles mg is
2.0
To determine the number of moles of oxygen gas needed to react with 4.0 moles of magnesium (Mg), we need to use the balanced chemical equation of the reaction between magnesium and oxygen. The balanced equation is:
2 Mg + O2 -> 2 MgO
From the equation, we can see that 2 moles of magnesium react with 1 mole of oxygen gas to produce 2 moles of magnesium oxide.
Therefore, we can set up a proportion using the given number of moles of magnesium (4.0 moles) to find the number of moles of oxygen gas:
(2 moles Mg / 1 mole O2) = (4.0 moles Mg / X moles O2)
Cross-multiplying gives:
2 moles Mg * X moles O2 = 4.0 moles Mg * 1 mole O2
X = (4.0 moles Mg * 1 mole O2) / 2 moles Mg
X = 2.0 moles O2
Therefore, 4.0 moles of magnesium will react with 2.0 moles of oxygen gas.
To determine the number of moles of oxygen gas needed to react with 4.0 moles of magnesium (Mg), we need to look at the balanced chemical equation for the reaction between magnesium and oxygen.
The balanced chemical equation for the reaction is as follows:
2 Mg + O2 -> 2 MgO
From this equation, we can see that 2 moles of magnesium react with 1 mole of oxygen gas to produce 2 moles of magnesium oxide.
So, for every 2 moles of magnesium, we need 1 mole of oxygen gas.
Since we have 4.0 moles of magnesium, we can set up a proportion:
2 moles Mg / 1 mole O2 = 4.0 moles Mg / X moles O2
Cross-multiplying the proportion, we get:
2 moles Mg * X moles O2 = 4.0 moles Mg * 1 mole O2
2X = 4.0
Dividing both sides by 2, we find:
X = 2.0 moles of oxygen gas
Therefore, 2.0 moles of oxygen gas are needed to react with 4.0 moles of magnesium.
Is there a formula with this question?
Mg + O2 ---> ?