if a mass of 2.4 g of magnesium is burnt in air, 4.0g of magnesium oxide is formed.
1- what kind of reaction is this ? explain your answer
b- what was the mass of oxygen that reacted with the magnesium? explain you answer
1) 2.30
2)2.30
1- The reaction between magnesium and oxygen to form magnesium oxide is a combustion reaction. In a combustion reaction, a substance reacts with oxygen to produce heat and light. In this case, magnesium is reacting with oxygen to form magnesium oxide.
b- To determine the mass of oxygen that reacted with the magnesium, we need to calculate the difference in mass between the initial magnesium and the final magnesium oxide.
Initial mass of magnesium = 2.4 g
Final mass of magnesium oxide = 4.0 g
The difference in mass between the two is the mass of oxygen that reacted.
Mass of oxygen = Final mass of magnesium oxide - Initial mass of magnesium
Mass of oxygen = 4.0 g - 2.4 g
Mass of oxygen = 1.6 g
Therefore, the mass of oxygen that reacted with the magnesium is 1.6 grams.
1- The reaction between magnesium and oxygen is a combustion reaction. In a combustion reaction, a substance reacts rapidly with oxygen to produce heat and light. In this case, magnesium reacts with oxygen in the air to form magnesium oxide (MgO). The reaction is represented by the following equation:
2Mg + O2 -> 2MgO
b- To determine the mass of oxygen that reacted with the magnesium, we need to use stoichiometry and the balanced equation. We know that 2.4g of magnesium reacted to form 4.0g of magnesium oxide. By comparing the coefficients of magnesium and magnesium oxide in the balanced equation (2:2), we can conclude that for every 2 moles of magnesium, 2 moles of magnesium oxide are formed.
To find the mass of oxygen, we first calculate the moles of magnesium that reacted:
moles of magnesium = mass of magnesium / molar mass of magnesium
moles of magnesium = 2.4g / 24.31 g/mol (molar mass of magnesium)
moles of magnesium = 0.0988 mol
Since 2 moles of magnesium oxide are formed for every 2 moles of magnesium, we know that the number of moles of magnesium oxide is also 0.0988 mol.
Now, we use stoichiometry to determine the molar ratio between magnesium oxide and oxygen. From the balanced equation, we can see that for every 2 moles of magnesium oxide, 1 mole of oxygen gas is required.
moles of oxygen = moles of magnesium oxide / ratio of moles of oxygen in the balanced equation
moles of oxygen = 0.0988 mol / 2
moles of oxygen = 0.0494 mol
Finally, we calculate the mass of oxygen by multiplying the number of moles by the molar mass of oxygen:
mass of oxygen = moles of oxygen × molar mass of oxygen
mass of oxygen = 0.0494 mol × 32.00 g/mol (molar mass of oxygen)
mass of oxygen = 1.58 g
Therefore, the mass of oxygen that reacted with the magnesium is approximately 1.58 grams.