Question

1. if 178.8 g of water is separated into hydrogen and oxygen gas, and the hydrogen gas has a mass of 20.0 g. what is the mass of the oxygen gas produced? 178.8g h₂o → 20g h₂ + g o₂ 4. from a laboratory process, a student collects 28.0 g of hydrogen and 224.0 g of oxygen. how much water was originally involved in the process? g h₂o → 28g h₂ + 224 g o₂ 5. a 10 - gram sample of iron reacts with oxygen to form 18.2 grams of ferric oxide. how many grams of oxygen reacted? 10g fe + g o₂ → 18.2g fe₂o₃

Explanation:

Step1: Apply law of conservation of mass

The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. So, the mass of reactants equals the mass of products.

Step2: Solve for mass in question 3

Let the mass of oxygen gas be $x$. We know that the mass of water is the sum of the mass of hydrogen gas and the mass of oxygen gas. So, $178.8 = 20.0+x$. Solving for $x$, we get $x=178.8 - 20.0=158.8$ g.

Step3: Solve for mass in question 4

Let the mass of water be $y$. According to the law of conservation of mass, $y=28.0 + 224.0=252.0$ g.

Step4: Solve for mass in question 5

Let the mass of oxygen be $z$. We have $10+z = 18.2$. Solving for $z$, we get $z=18.2 - 10=8.2$ g.

Answer:

1. 158.8 g
2. 252.0 g
3. 8.2 g