Question

1SO2 + 3H2 = 1H2S + 2H2O
products: 2H2S, 4H2O
leftovers: 3SO2, 2H2
what are the reactants?

Answer 1

To determine the reactants based on the information provided, we can start by analyzing the chemical reaction you provided:

\[ \text{1 SO}_2 + 3 \text{H}_2 \rightarrow \text{1 H}_2\text{S} + 2 \text{H}_2\text{O} \]

We see that 1 mole of sulfur dioxide (SO₂) reacts with 3 moles of hydrogen gas (H₂) to produce 1 mole of hydrogen sulfide (H₂S) and 2 moles of water (H₂O).

You mentioned the products as 2 H₂S and 4 H₂O, along with leftovers of 3 SO₂ and 2 H₂.

From the stoichiometry of the reaction, let's analyze it step-by-step to find out how many moles of reactants were used:

1. Given products:
- 2 moles of H₂S
- 4 moles of H₂O

2. From the reaction equation:
- To produce 2 moles of H₂S, you need 2 moles of SO₂ and 6 moles of H₂ (because for each mole of H₂S produced, 1 mole of SO₂ and 3 moles of H₂ are required).

3. However, there are leftovers:
- 3 moles of SO₂ (which means only 1 mole was used).
- 2 moles of H₂ (which means no H₂ was consumed, contradicting the need for 6 moles).

Based on the original reaction and the information provided, the intended reactants, to achieve the stated products while adhering to the reaction stoichiometry, would be:

- 2 moles of SO₂ (only 1 is stated)
- 6 moles of H₂ (only 2 is stated)

However, if we match to the number of leftovers, we conclude:

1 mole SO₂ was consumed, and none of the H₂ was consumed, indicating that the actual reactants cannot produce the stated products with the leftovers.

So, the reactants in the reaction you have described (before leftovers) would be:

\[ \text{Reactants: 1 SO}_2 \text{ and } 3 \text{H}_2 \]

This would mean that the reaction was either not completed, or there’s an inconsistency in the quantities of products and leftovers you provided.