1. Calculate the AH°rxn for the following reaction. (AH°f [SiO2(s)] = -910.9 kJ/mol; AH°f [SiC14(g)] = -657.0 kJ/mol; AHᵒf [HCI(g)] = -92.3 kJ/mol; AH°f [H2O(g)] = -241.8 kJ/mol) SiO2 (s) + 4HCI(g) → SiC14(g) + 2H2O(g) 06 A)-137.4 kJ B)-139.5 kJ C) 104.4 kJ D) 139.5 kJ E)-104.4 kJ [(-6570)+2(-241.8)]-(923) + (-910.9)] -1140.6-(-1280.1) = 139.5 K)
1. Calculate the AH°rxn for the following reaction. (AH°f [SiO2(s)] = -910.9 kJ/mol; AH°f [SiC14(g)] = -657.0 kJ/mol; AHᵒf [HCI(g)] = -92.3 kJ/mol; AH°f [H2O(g)] = -241.8 kJ/mol) SiO2 (s) + 4HCI(g) → SiC14(g) + 2H2O(g) 06 A)-137.4 kJ B)-139.5 kJ C) 104.4 kJ D) 139.5 kJ E)-104.4 kJ [(-6570)+2(-241.8)]-(923) + (-910.9)] -1140.6-(-1280.1) = 139.5 K)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![Experimental determination
qloss + again = 0
Bond energies (D)
Ο
Draw lewis structures & use stoich!
Standard Enthalpy of formation AHºf
Hess's Law and AH
om 11:05
Methods for knowing/ approximating the AHxn
9rxn & AHrxn
q = mcAT
A)-137.4 kJ
B)-139.5 kJ
C) 104.4 kJ
D) 139.5 kJ
E)-104.4 kJ
AHxn
Name
qrxn
moles Limiting
ΔΗχη = Σ D bonds broken - Σ D bonds formed
AHᵒrn = ΣAHᵒf products - ZAH°, reactants
Claire Dutty
Sum of multiple step process = 1 step process
Flip elementary formation reactions to align with final balanced equation of interest, flip AH
Multiply elementary formation reactions to align with final balanced equation, multiply AH
Cancel intermediates and sum up AH to find AH<rxn
lom
Standard Enthalpy of formation and AHrxn
1. Calculate the AH°rxn for the following reaction. (AH°f [SiO2(s)] = -910.9 kJ/mol; AH°f [SiC14(g)] = -657.0
kJ/mol; AH°f [HCl(g)] = -92.3 kJ/mol; AH°f [H2O(g)] = -241.8 kJ/mol)
SiO2 (s) + 4HCI(g) → SiC14(g) + 2H2O(g) omil 0.3s8
is
[(-657.0)+2(-241.8)]-(923) + (-910.9)]
-1140.6 -(-1280.1) = 139.5 K)
2. Nitric acid, which is among the top 15 chemicals produced in the United States, was first prepared over 1200
years ago by heating naturally occurring sodium nitrate (called saltpeter) with sulfuric acid and collecting the
S](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5a487c5b-631b-4d04-995d-e7c019732a55%2F326bff5e-e968-40ef-b2bb-57274238bda5%2Fmjt8i0b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Experimental determination
qloss + again = 0
Bond energies (D)
Ο
Draw lewis structures & use stoich!
Standard Enthalpy of formation AHºf
Hess's Law and AH
om 11:05
Methods for knowing/ approximating the AHxn
9rxn & AHrxn
q = mcAT
A)-137.4 kJ
B)-139.5 kJ
C) 104.4 kJ
D) 139.5 kJ
E)-104.4 kJ
AHxn
Name
qrxn
moles Limiting
ΔΗχη = Σ D bonds broken - Σ D bonds formed
AHᵒrn = ΣAHᵒf products - ZAH°, reactants
Claire Dutty
Sum of multiple step process = 1 step process
Flip elementary formation reactions to align with final balanced equation of interest, flip AH
Multiply elementary formation reactions to align with final balanced equation, multiply AH
Cancel intermediates and sum up AH to find AH<rxn
lom
Standard Enthalpy of formation and AHrxn
1. Calculate the AH°rxn for the following reaction. (AH°f [SiO2(s)] = -910.9 kJ/mol; AH°f [SiC14(g)] = -657.0
kJ/mol; AH°f [HCl(g)] = -92.3 kJ/mol; AH°f [H2O(g)] = -241.8 kJ/mol)
SiO2 (s) + 4HCI(g) → SiC14(g) + 2H2O(g) omil 0.3s8
is
[(-657.0)+2(-241.8)]-(923) + (-910.9)]
-1140.6 -(-1280.1) = 139.5 K)
2. Nitric acid, which is among the top 15 chemicals produced in the United States, was first prepared over 1200
years ago by heating naturally occurring sodium nitrate (called saltpeter) with sulfuric acid and collecting the
S
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