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) + 2Cl2(g) --> SnCl4(l)
ΔH°rxn = -511.3 kJ/mol
ΔU°rxn = -506.3

H2(g) + Cl2(g) --> 2HCl(g)
ΔH°rxn = -184.6 kJ/mol
ΔU°rxn = ?

I know ΔU°rxn = q + work
q = ΔH°rxn

How do I find work for the second reaction?

4 answers

Since the number of moles of the reactants is 1+1 and the number of moles of the product is 2, they are equal which means that the change in the number of moles is zero. This means that ΔU°rxn is going to be equal to ΔH°rxn. ΔU°rxn= -184.6
Avery is correct
The standard internal energy change for a reaction can be symbolized as Δ𝑈∘rxn or Δ𝐸∘rxn . For each reaction equation, calculate the energy change of the reaction at 21 ∘C and 1.00 bar .
2H2(g)+O2(g)⟶2H2O(l)Δ𝐻∘rxn=−561.2 kJ/mol
thog
Similar Questions
    1. answers icon 16 answers
  1. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)standard enthalpy: -133.5 Find the change in internal energy for this reaction. Enter in
    1. answers icon 7 answers
  2. Use standard enthalpies of formation to determine ƒ¢Horxn for:2NH3(g) + 3O2(g) + 2CH4(g) �¨ 2HCN(g) + 6H2O(g) in kilojoules.
    1. answers icon 0 answers
    1. answers icon 2 answers
more similar questions