The standard internal energy change for a reaction can be symbolized as δu∘rxn or e∘rxn. for each reaction equation, calculate the energy change of the reaction at 25∘c and 1.00 bar.
2h2(g) + o2(g) ⟶ 2h2o(l) δh∘rxn= −571.6kj/mol

h2(g) + cl2(g) ⟶ 2hcl(g) δh∘rxn= −184.6kj/mol

answer:

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.

a) sn (s) + 2cl2 (g) -> sncl4 (l)

δh°rxn (kj·mol–1): -511.3

b) h2 (g) + cl2 (g) -> 2hcl (g)

δh°rxn (kj·mol–1): -184.6

according to kinetic-molecular theory, the following would not be considered an ideal gas:

a gas at very low volumes, when gas particles are very close together

a gas at very low temperatures, when gas particles have very little kinetic energy a gas

a gas with highly polar molecules that have very strong intermolecular forces

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