Question

During the combustion of hydrogen sulfide, 500g of water are produced. How many grams of hydrogen sulfide were consumed? How many grams of oxygen were consumed?

a) Hydrogen sulfide consumed: 100g, Oxygen consumed: 400g
b) Hydrogen sulfide consumed: 400g, Oxygen consumed: 100g
c) Hydrogen sulfide consumed: 300g, Oxygen consumed: 200g
d) Hydrogen sulfide consumed: 200g, Oxygen consumed: 300g

Answer 1

During the combustion of hydrogen sulfide, 500g of water are produced. The grams of hydrogen sulfide consumed are 500g, and the grams of oxygen consumed are 250g.

Step-by-step explanation:

To determine the grams of hydrogen sulfide consumed and oxygen consumed during the combustion reaction, we need to use the balanced chemical equation:

2H₂S (g) + 3O₂ (g) → 2SO₂ (g) + 2H₂O(g)

From the equation, we can see that for every 2 moles of H₂S consumed, 2 moles of H₂O are produced. This means that the number of moles of hydrogen sulfide consumed is the same as the number of moles of water produced. Since 500g of water are produced, this means that 500g of hydrogen sulfide were consumed.

Similarly, from the equation, we can see that for every 3 moles of oxygen consumed, 2 moles of H₂O are produced. This means that the number of moles of oxygen consumed is half of the number of moles of water produced. Since 500g of water are produced, this means that 250g of oxygen were consumed.

Therefore, the correct answer is: Hydrogen sulfide consumed: 500g, Oxygen consumed: 250g.