The enthalpy change for the reaction using standard enthalpies has to be determined Concept Introduction: The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states. Enthalpy change for the reaction Δ r H 0 = ΣnΔ f H 0 (products) - ΣnΔ f H 0 (reactants)
The enthalpy change for the reaction using standard enthalpies has to be determined Concept Introduction: The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states. Enthalpy change for the reaction Δ r H 0 = ΣnΔ f H 0 (products) - ΣnΔ f H 0 (reactants)
The enthalpy change for the reaction using standard enthalpies has to be determined
Concept Introduction:
The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.
Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)
(a)
Expert Solution
Explanation of Solution
Given,
ΔfH0(C)= 0 KJ/mol
ΔfH0(H2O)=-241.8kJ/mol
ΔfH0(CO)=-110.54kJ/mol
ΔfH0(H2)=0J/mol
Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)
ΔrH° =(-110.54+0)-(0+-241.8)
ΔrH0=131.26 kJ/mol
So, the change in enthalpy of the reaction is 131.3kJ/mol
(b)
Interpretation Introduction
Interpretation:
The nature of the reaction has to be identified.
Concept Introduction:
The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.
Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)
(b)
Expert Solution
Explanation of Solution
Given,
ΔfH0(C)= 0 KJ/mol
ΔfH0(H2O)=-241.8kJ/mol
ΔfH0(CO)=-110.54kJ/mol
ΔfH0(H2)=0J/mol
Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)
ΔrH° =(-110.54+0)-(0+-241.8)
ΔrH0=131.26 kJ/mol
The change in enthalpy is +131.3kJ/mol, so it is endothermic reaction.
(c)
Interpretation Introduction
Interpretation:
The enthalpy change if 1000.0kg of carbon converted to water gas has to be calculated.
Concept Introduction:
The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.
Enthalpy change for the reaction ΔrH0=ΣnΔfH0(products)-ΣnΔfH0(reactants)
(c)
Expert Solution
Explanation of Solution
The change in enthalpy is +131.3kJ/mol,
Heat evolved when 1000Kg of carbon is converted to coal:
Vnk the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest bolling
point, choose 2 next to the substance with the next highest boiling point, and so on.
substance
C
D
chemical symbol,
chemical formula
or Lewis structure.
CH,-N-CH,
CH,
H
H 10: H
C-C-H
H H H
Cale
H 10:
H-C-C-N-CH,
Bri
CH,
boiling point
(C)
Сен
(C) B
(Choose
Please help me find the 1/Time, Log [I^-] Log [S2O8^2-], Log(time) on the data table. With calculation steps. And the average for runs 1a-1b. Please help me thanks in advance. Will up vote!
Q1: Answer the questions for the reaction below:
..!! Br
OH
a) Predict the product(s) of the reaction.
b) Is the substrate optically active? Are the product(s) optically active as a mix?
c) Draw the curved arrow mechanism for the reaction.
d) What happens to the SN1 reaction rate in each of these instances:
1. Change the substrate to
Br
"CI
2. Change the substrate to
3. Change the solvent from 100% CH3CH2OH to 10% CH3CH2OH + 90% DMF
4. Increase the substrate concentration by 3-fold.
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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