Use Table 8.3 to obtain Δ H ° for the following chemical equations: (a) Zn ( s ) + 2 H + ( a q ) → Zn 2 + ( a q ) + H 2 ( g ) (b) 2H 2 S ( g ) + 3 O 2 ( g ) → 2 SO 2 ( g ) + 2 H 2 O ( g ) (c) 3Ni ( s ) + 2 NO 3 − ( a q ) + 8H + ( a q ) → 3 Ni 2 + ( a q ) + 2 NO ( g ) + 4 H 2 O ( l )
Use Table 8.3 to obtain Δ H ° for the following chemical equations: (a) Zn ( s ) + 2 H + ( a q ) → Zn 2 + ( a q ) + H 2 ( g ) (b) 2H 2 S ( g ) + 3 O 2 ( g ) → 2 SO 2 ( g ) + 2 H 2 O ( g ) (c) 3Ni ( s ) + 2 NO 3 − ( a q ) + 8H + ( a q ) → 3 Ni 2 + ( a q ) + 2 NO ( g ) + 4 H 2 O ( l )
Use Table 8.3 to obtain ΔH° for the following chemical equations:
(a)
Zn
(
s
)
+
2
H
+
(
a
q
)
→
Zn
2
+
(
a
q
)
+
H
2
(
g
)
(b)
2H
2
S
(
g
)
+
3
O
2
(
g
)
→
2
SO
2
(
g
)
+
2
H
2
O
(
g
)
(c)
3Ni
(
s
)
+
2
NO
3
−
(
a
q
)
+
8H
+
(
a
q
)
→
3
Ni
2
+
(
a
q
)
+
2
NO
(
g
)
+
4
H
2
O
(
l
)
Expert Solution
Interpretation Introduction
(a)
Interpretation:
The value of ΔH° for the given chemical equation needs to be calculated.
Zn (s) + 2H+(aq)→Zn2+(aq) + H2(g)
Concept introduction:
The change in standard enthalpy for a reaction, ΔH0 is given in terms of the difference in the standard enthalpy of formation of the products and that of reactants.
The value of ΔH° for the given chemical equation needs to be calculated.
2H2S(g) + 3O2(g)→2SO2(g) + 2H2O(g)
Concept introduction:
The change in standard enthalpy for a reaction, ΔH0 is given in terms of the difference in the standard enthalpy of formation of the products and that of reactants.
The change in standard enthalpy for a reaction, ΔH0 is given in terms of the difference in the standard enthalpy of formation of the products and that of reactants.
Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon:
C(s) + H2 O(g) ⟶ CO(g) + H2(g).
(a) Assuming that coke has the same enthalpy of formation as graphite, calculate ΔH° for this reaction.
(b) Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst: 2H2(g) + CO(g) ⟶ CH3 OH(g).
Under the conditions of the reaction, methanol forms as a gas. Calculate ΔH° for this reaction and for the condensation of gaseous methanol to liquid methanol.
(c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g).
Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon: C(s) + H2 O(g) ⟶ CO(g) + H2(g).(a) Assuming that coke has the same enthalpy of formation as graphite, calculate ΔH°298 for this reaction.(b) Methanol, a liquid fuel that could possibly replace gasoline, can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst: 2H2(g) + CO(g) ⟶ CH3 OH(g).Under the conditions of the reaction, methanol forms as a gas. Calculate ΔH°298 for this reaction and for the condensation of gaseous methanol to liquid methanol.(c) Calculate the heat of combustion of 1 mole of liquid methanol to H2O(g) and CO2(g).
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Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY