When 24g of Magnesium reacts with oxygen gas the only product is magnesium oxide. If 40g magnesuim is produced how much oxygen was consumed?
2Mg + O2 ==> 2MgO
You must mean if 40 g magnesium OXIDE are produced and you must be using 24 for the atomic mass Mg and 40 as molar mass MgO. In those circumstances.
mols Mg = 24/24 = 1 mol and that will produce 40 g MgO.
mols O2 consumed = 40g MgO x (1 mol O2/2 mol MgO) = 40 x 1/2 = 20 mols O2.
Then grams O2 = mols x molar mass.
THE PRODUCT OF MAGNESIUM +OXYGEN LOOK LIKE IS (soft /hard) IN A FORM OF A (LIQUID /SOLID /GAS) AND IS (WHITE /BLACK /YELLOW) IN COLOUR
To determine how much oxygen was consumed in the reaction, we need to use the concept of the law of conservation of mass. According to this law, in a chemical reaction, the total mass of the reactants must be equal to the total mass of the products.
In this case, we are given that 24g of magnesium reacted with oxygen gas to produce 40g of magnesium oxide. Let's assume that x grams of oxygen gas were consumed in the reaction.
The balanced chemical equation for the reaction is:
2Mg + O2 → 2MgO
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.
To calculate the amount of oxygen consumed, we'll use the molar masses of magnesium (24.31 g/mol) and oxygen (16.00 g/mol):
For magnesium:
Mass = moles × molar mass
24g = (2 moles of Mg) × (24.31 g/mol)
24g = 48.62 g
So, 2 moles of magnesium weigh 48.62 grams.
For oxygen:
Mass = moles × molar mass
x g = (1 mole of O2) × (32.00 g/mol)
x g = 32.00 g
So, 1 mole of oxygen gas weighs 32.00 grams.
We know that the total mass of magnesium oxide produced is 40g.
Total mass of products = mass of magnesium oxide
40g = (2 moles of MgO) × (24.31 g/mol + 16.00 g/mol)
Simplifying the equation:
40g = 2(40.31 g/mol)
40g = 80.62 g/mol
Now, we can find the number of moles of oxygen used:
Total mass of reactants (magnesium and oxygen) = Total mass of products
48.62 g + x g = 80.62 g
x g = 80.62 g - 48.62 g
x g = 32 g
Therefore, 32 grams of oxygen gas were consumed in the reaction.