Relate Enthalpy to Reactions
Chemistry · Flashcards · Application
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QUESTION
Which is more exothermic: a reaction with
Δ
H
=
−
50
k
J
\Delta H=-50\ \mathrm{kJ}
Δ
H
=
−
50
kJ
or
Δ
H
=
−
10
k
J
\Delta H=-10\ \mathrm{kJ}
Δ
H
=
−
10
kJ
?
QUESTION
Calculate
Δ
H
r
x
n
∘
\Delta H_{rxn}^\circ
Δ
H
r
x
n
∘
given
∑
n
Δ
H
f
∘
(
prod
)
=
−
120
k
J
\sum n\Delta H_f^\circ(\text{prod})=-120\ \mathrm{kJ}
∑
n
Δ
H
f
∘
(
prod
)
=
−
120
kJ
and
∑
n
Δ
H
f
∘
(
react
)
=
−
300
k
J
\sum n\Delta H_f^\circ(\text{react})=-300\ \mathrm{kJ}
∑
n
Δ
H
f
∘
(
react
)
=
−
300
kJ
.
QUESTION
What is
Δ
H
\Delta H
Δ
H
for a reaction that releases
250
k
J
250\ \mathrm{kJ}
250
kJ
of heat at constant pressure?
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ANSWER
Δ
H
=
−
250
k
J
\Delta H=-250\ \mathrm{kJ}
Δ
H
=
−
250
kJ
. Heat released means negative enthalpy change.
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