Question

1. in a chemical reaction, 64g of zinc is reacted with excess oxygen to form 80g of zinc oxide. how much oxygen is used in this reaction? (1 pt)

Explanation:

Step1: Apply the law of conservation of mass

The law of conservation of mass states that in a chemical reaction, the total mass of reactants is equal to the total mass of products.
Let the mass of oxygen be \(m\). The mass of reactants is \(m_{Zn}+m\) (mass of zinc + mass of oxygen), and the mass of product is \(m_{ZnO}\) (mass of zinc oxide). So, \(m_{Zn}+m = m_{ZnO}\).

Step2: Solve for the mass of oxygen

We know \(m_{Zn} = 64g\) and \(m_{ZnO}=80g\). Rearranging the equation \(m_{Zn}+m = m_{ZnO}\) for \(m\), we get \(m=m_{ZnO}-m_{Zn}\).
Substitute the values: \(m = 80g - 64g\).

Answer:

\(16g\)