The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn (s) + Cl2 (g) - - - > SnCl4 (l) + H (KJmol) - 511.3. H2 (g) + Cl2 (g) - - - > 2HCl (g) + H (KJmol) - 184.6

Question

Armando Contreras

Chemistry

20 March, 02:25

The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate the energy change of the reaction at 25 °C and 1.00 bar. Sn (s) + Cl2 (g) - - - > SnCl4 (l) + H (KJmol) - 511.3. H2 (g) + Cl2 (g) - - - > 2HCl (g) + H (KJmol) - 184.6

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Hana Benton · Answer 1

The formula for ΔU°rxn is: ΔU°rxn = H - PV. Assuming ideal gas, it could also be: ΔU°rxn = H - RT.

For the first reaction:

ΔU°rxn = (-511.3 kJ/mol) - (0.008314 J/mol-K) (25+273 K) = - 513.78 kJ/mol

For the second reaction:

ΔU°rxn = (-184.6 kJ/mol) - (0.008314 J/mol-K) (25+273 K) = - 187.08 kJ/mol