Chemistry Stoichiometry Solution: How many molecules of H2S are required to form 79....

🤓 Based on our data, we think this question is relevant for Professor Marzal's class at UCF.

Solution: 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 H2SB) 2.44 × 1023 molecules H2SC) 5.06 × 1025 molecules H2SD) 3.17 × 1025 molecules H2SE) 9.89 × 1023 molecules H2S

Problem

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

Solution

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 H2(Avogadro’s number)  Molecules of H2S


Solution BlurView Complete Written Solution