🤓 Based on our data, we think this question is relevant for Professor Marzal's class at UCF.
How many molecules of H2S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO2.
2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(l)
A) 1.48 × 1024 molecules H2S
B) 2.44 × 1023 molecules H2S
C) 5.06 × 1025 molecules H2S
D) 3.17 × 1025 molecules H2S
E) 9.89 × 1023 molecules H2S
We’re being asked to calculate the number of H2S molecules required to form 79.0 g sulfur. Since SO2 is in excess, we can simply ignore it in our calculations. The flow for this problem will be like this:
Mass of S (molar mass of S) → Moles of S (mole-to-mole comparison) → Moles of H2S (Avogadro’s number) → Molecules of H2S