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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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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

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