Question

3H2S + 2FeCl3 = Fe2S3 + 6HCl

a. How many grams of Fe2S3 can be prepared from 11.4 mL of 0.089 M FeCl3?

b. How many mL of H2S at 0.875 atm and 25C are required to consume 11.4 mL of 0.089 M FeCl3?

c. What is the ionic and net ionic equations?

Answer 1

a) Number of moles of FeCl3 = Volume of solution(in L) * molarity

=> 11.4/1000 * 0.089

=> 1.0146 * 10^(-3) moles

2 moles of FeCl3 makes 1 mole of Fe2S3

Moles of Fe2S3 produced = 1.0146 * 10^(-3) moles/2 = 5.073 * 10^(-4) moles

Molar mass of Fe2S3 = 2 * 55.845 + 3 * 32 = 207.9 gm/mol

Mass of Fe2S3 produced = 5.073 * 10^(-4) moles * 207.9 gm/mol = 0.1054 gms

b) 3 moles of H2S react with 2 moles of FeCl3

Moles of H2S required = 1.0146 * 10^(-3) moles * 3/2 = 1.5219 * 10^(-3) moles

Using ideal gas equation

PV = nRT

0.875 * V = 1.5219 * 10^(-3) * 0.0821 * 298

V = 42.553 mL

c) The states of the various products are not given, please check the question and get to back with me the same for writing ionic and net-ionic equation