Answer to Question #192168 in General Chemistry for Jade

Question #192168

2) Calculate the Δ

Δ

H value heat for the following reaction: Ag2S(s)  + 2 HCl(g) -->  2 AgCl(s) + H2S(g) Δ

Δ

H = ? kJ/mol Solve by writing formation equations for each reactant and product and using the Δ

Δ

H values for each.


1
Expert's answer
2021-05-21T02:33:38-0400

The given reaction is-

Ag2S(S) +2HCl(g) →2AgCl(S) +H2S(g)


Now, independent reactions are:

2Ag++S2-→Ag2S(s);  ∆Hf=−31.8 kJ/mol

H++Cl-→HCl(g);  ∆Hf=−92.3 kJ/mol

Ag++Cl-→AgCl(s);  ∆Hf=−127.0 kJ/mol

2H++S2-→H2S(g);  ∆Hf=−20.6 kJ/mol


Therefore, the enthalpy change of reaction can be given as follows:

∆Hrxn=Σn∆Hf(Products)−Σm∆Hf(Reactants)


=2∆Hf(AgCl(s))+1∆Hf(H2S(g))]

−[1∆Hf(Ag2S(s))+2∆Hf(HCl(g))]

=[2×(−127.0 kJ/mol)+1×(−20.6 kJ/mol)]

−[1×(−31.8 kJ/mol)+2×(−92.3 kJ/mol)]


=[-254 kJ/mol−20.6 kJ/mol]−[−31.8 kJ/mol−184.6 kJ/mol]

=[-274.6 kJ/mol−(−216.4 kJ/mol)]

=[−274.6 kJ/mol+216.4 kJ/mol]

=−58.2 kJ/mol



Answer: ΔH value heat for the following reaction:


Ag2S(S) +2HCl(g) →2AgCl(S) +H2S(g)

 is -58.2 kJ/mol.



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