Ask Question
2 June, 12:03

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

+4
Answers (1)
  1. 2 June, 13:41
    0
    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
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “The standard internal energy change for a reaction can be symbolized as ΔU°rxn or ΔE°rxn. For the following reaction equations, calculate ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers