Question

As shown in the equation below, 25g of oxygen gas (0-2) reacts with 10g 2 points

of hydrogen gas (H-2) to create water (H-20). What will be the expected
mass of the product (water) in this equation? O₂ + 2H₂ – 2H₂0.

Answer 1

The expected mass of water produced from the reaction of 25g of oxygen gas and 10g of hydrogen gas, according to the law of conservation of mass and the stoichiometry of the balanced chemical equation, would be 35g.

Step-by-step explanation:

The question is asking about the expected mass of water produced from the reaction of oxygen and hydrogen gases based on the given balanced chemical equation. It's important to understand the law of conservation of mass, which states that mass is neither created nor destroyed in a chemical reaction. Therefore, the mass of products in a reaction is always equal to the mass of the reactants.

According to the balanced chemical equation 2H₂(g) + O₂(g) → 2H₂O(l), two moles of hydrogen gas (H₂) react with one mole of oxygen gas (O₂) to produce two moles of water (H₂O). Given that hydrogen and oxygen are reacting in the given masses (25g of O₂ and 10g of H₂) and assuming that nothing else is involved in the reaction and it goes to completion, the mass of water produced would be the sum of the masses of the reactants, which is 25g + 10g = 35g.

So, based on the provided information and the stoichiometry of the balanced equation, the expected mass of water (H₂O) produced would be 35g.