Question

Consider the reaction 2H₂(g)+O₂(g)→2H₂O(l) What is the mass of water, H₂O(l), produced when 5.50 g of O₂(g) reacts with excess H₂(g)?

Answer 1

The mass of water produced when 5.50 g of O₂ reacts with excess H₂ is 3.10 g.

Step-by-step explanation:

In the given reaction, 2H₂(g)+O₂(g)→2H₂O(l), the coefficients of the reactants and products indicate the ratio of moles. To find the mass of water produced, we need to calculate the number of moles of O₂ and then use the molar mass of water to convert moles to grams.

First, calculate the number of moles of O₂ using its molar mass:

1. Find the molar mass of O₂: 1 mol O₂ = 32.0 g O₂
2. Calculate the number of moles of O₂: moles of O₂ = mass of O₂ / molar mass of O₂
3. Substitute the given values: moles of O₂ = 5.50 g / 32.0 g/mol = 0.172 mol O₂

Since the balanced equation shows that 2 moles of H₂O(l) are produced for every 1 mole of O₂, we can multiply the number of moles of O₂ by the molar mass of water to find the mass of water produced:

1. Find the molar mass of H₂O: 1 mol H₂O = 18.02 g H₂O
2. Calculate the mass of water produced: mass of water = moles of O₂ * molar mass of H₂O
3. Substitute the calculated value: mass of water = 0.172 mol O₂ * 18.02 g/mol = 3.10 g H₂O

Therefore, the mass of water produced when 5.50 g of O₂(g) reacts with excess H₂(g) is 3.10 g.