Question

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.09 g of magnesium

ribbon burns with 8.75 g of oxygen, a bright, white light and a white, powdery product are formed.
Enter the balanced chemical equation for this reaction. Be sure to include all physical states.
equation:
What is the limiting reactant?
magnesium
oxygen

If the percent yield for the reaction is 90.3%, how many grams of product were
formed?


How many grams of the excess reactant remain?

Answer 1

The balanced chemical equation for the reaction between magnesium and oxygen is 2Mg (s) + O₂(g) → 2MgO (s). Magnesium is the limiting reactant. To calculate the mass of the product formed, use the moles of the limiting reactant, molar mass of the product, and percent yield. Subtract the mass consumed by the limiting reactant to find the grams of excess reactant remaining.

Step-by-step explanation:

The balanced chemical equation for the reaction between magnesium and oxygen is:

2Mg (s) + O₂(g) → 2MgO (s)

In the given reaction, magnesium is the limiting reactant because it produces less MgO compared to oxygen. To calculate the mass of the product formed, we need to determine the moles of the limiting reactant and use stoichiometry. Assuming a 90.3% percent yield, we can calculate the mass of the product formed using the formula:

mass of product = moles of limiting reactant × molar mass of product × percent yield

To find the grams of excess reactant remaining, subtract the mass consumed by the limiting reactant from the total mass of the excess reactant given.

Answer 2

the answer is: Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.51 g of magnesium ribbon burns with 8.50 g of oxygen, a bright, white light and a white, powdery product are formed