A sample of 50g of ferric chloride reacts with 40g of hydrogen sulphide . Determine the amount of hydrogen chloride formed in the reaction ???

Dear Student,

The balanced chemical reaction for ferric chloride with hydrogen sulphide is:

$$\begin{gathered} 2FeC{l}_3+2H_{2}S \to Fe{S}_2+FeC{l}_2+4HCl \\ from the equation it can be seen that \\ 2 mole of FeC{l}_3 and 2 mole of H_{2}S is required to react completely \\ i.e. for 2\times 162.2g of FeC{l}_3 \to 2\times 34g of H_{2}S is required \\ for 50g of FeC{l}_3 \to \frac{2\times 34}{2\times 162.2g}\times 50 = 10.5 g of H_{2}S is required \\ So, in the given reac\tan ts, FeC{l}_3 is the limiting reagent as it is less in amount and so the amount of product will depend on this only \\ now, 2 mole of FeC{l}_3 \to 4 mole of HCl \\ i.e. 2\times 162.2g of FeC{l}_3 \to 4\times 36.5g of HCl \\ 50g of FeC{l}_3 \to \frac{4\times 36.5}{2\times 162.2}\times 50g = 22.5g of HCl \\ Therefore, 22.5g of HCl will be formed in the reaction. \end{gathered}$$


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