# chemistry

posted by jake

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?

1. Avery

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

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