Part D Application of Hess's Law a. Write in your experimentally-derived thermochemical equations. (1) (2) enthalpy values in the following Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g) Mg0(s) + 2 HCl(aq) → MgCl₂(aq) + H₂O(1) AH₁ = ΔΗ, = b. Use Hess's Law to get AH3 for reaction (3) from AH₁ and AH₂. (3) Mg(s) + H₂O(1)→➜ MgO(s) + H₂(g) AH3 = c. Now calculate AH3 from standard molar enthalpies of formation found in the thermodynamic tables in the appendix.
Part D Application of Hess's Law a. Write in your experimentally-derived thermochemical equations. (1) (2) enthalpy values in the following Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g) Mg0(s) + 2 HCl(aq) → MgCl₂(aq) + H₂O(1) AH₁ = ΔΗ, = b. Use Hess's Law to get AH3 for reaction (3) from AH₁ and AH₂. (3) Mg(s) + H₂O(1)→➜ MgO(s) + H₂(g) AH3 = c. Now calculate AH3 from standard molar enthalpies of formation found in the thermodynamic tables in the appendix.
Chemistry by OpenStax (2015-05-04)
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Chapter5: Thermochemistry
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![Part D Application of Hess's Law
a. Write in your experimentally-derived
thermochemical equations.
(1)
(2)
enthalpy values in the following
ΔΗ,
=
ΔΗ, =
Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g)
Mg0(s) + 2 HCl(aq) → MgCl₂(aq) + H₂O(1)
b. Use Hess's Law to get AH3 for reaction (3) from AH₁ and AH₂.
(3) Mg(s) + H₂O(1)→ MgO(s) + H₂(g)
AH3 =
c. Now calculate AH3 from standard molar enthalpies of formation found in the
thermodynamic tables in the appendix.
d. Discussion: Compare your experimental value of AH3 with the value calculated
from the thermodynamic tables. Can you explain why they shouldn't be exactly
the same?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4295bf62-da14-49f1-b3bf-6e678bc68de3%2F778c1e20-dd0f-4035-97db-6a1e102a6cd8%2Fqy7a00b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Part D Application of Hess's Law
a. Write in your experimentally-derived
thermochemical equations.
(1)
(2)
enthalpy values in the following
ΔΗ,
=
ΔΗ, =
Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g)
Mg0(s) + 2 HCl(aq) → MgCl₂(aq) + H₂O(1)
b. Use Hess's Law to get AH3 for reaction (3) from AH₁ and AH₂.
(3) Mg(s) + H₂O(1)→ MgO(s) + H₂(g)
AH3 =
c. Now calculate AH3 from standard molar enthalpies of formation found in the
thermodynamic tables in the appendix.
d. Discussion: Compare your experimental value of AH3 with the value calculated
from the thermodynamic tables. Can you explain why they shouldn't be exactly
the same?
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