CHE 106 Lecture Notes - Lecture 19: Enthalpy, Joule

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CHE 106 Lecture 18: Calorimetry

CHE 106 Lecture Notes - Lecture 19: Enthalpy, Joule

CHE 106 Lecture 20: Lecture 20: Chapter 6: Section 5 -7

Document Summary

Lecture 17 made from its constituent elements in elemental forms. Enthalpy of formation: defined as enthalpy change for reaction in which a compound is. Standard enthalpy of formation: : enthalpy change for formation of one mol of a. Formation reaction: reaction that produces one mol of a single product out of elements in their standard state; some may use fractional stoichiometric coefficients: standard enthalpy depends on state, ex. Water= -285. 8 kj/mol; water vapor= -241. 8 kj/mol: higher thermodynamic measure means substance is less stable, ex. Diamond is +1. 897 kj/mol, meaning grahite is more stable than diamond. Law of summation of heats of formation: enthalpy=total formation of energy of products- reactants. Electricity and (fossil) fuels are most common sources of energy in society. Food is fuel source for body; energy released from one gram of food is combusted is its fuel value: one gram of glucose yields 15. 6 kj.

Related Questions

What is the balanced chemical equation for the reaction used to calculate ÎHâf of CaCO3(s)? If fractional coefficients are required, enter them as a fraction (i.e. 1/3). Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution. Express your answer as a chemical equation. The standard enthalpy of formation (ÎHâf) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of 25 âC , and all the species present at a concentration of 1 M . A "standard enthalpies of formation table" containing ÎHâf values might look something like this: Substance ÎHâf H(g) 218 kJ/mol H2(g) 0 kJ/mol Ca(s) 0 kJ/mol Ca2+(aq) â543 kJ/mol C(g) 71 kJ/mol C(s) 0 kJ/mol N(g) 473 kJ/mol O2(g) 0 kJ/mol O(g) 249 kJ/mol S2(g) 129 kJ/mol

The standard enthalpy of formation (ÎHâf) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of25 âC , and all the species present at a concentration of 1 M . A "standard enthalpies of formation table" containing ÎHâf values might look something like this:

Substance	ÎHâf
H(g)	218 kJ/mol
H2(g)	0 kJ/mol
Ca(s)	0 kJ/mol
Ca2+(aq)	â543 kJ/mol
C(g)	71 kJ/mol
C(s)	0 kJ/mol
N(g)	473 kJ/mol
O2(g)	0 kJ/mol
O(g)	249 kJ/mol
S2(g)	129 kJ/mol

Part A

What is the balanced chemical equation for the reaction used to calculate ÎHâf of CaCO3(s)?

If fractional coefficients are required, enter them as a fraction (i.e. 1/3). Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively without indicating allotropes. Use (aq) for aqueous solution.

Express your answer as a chemical equation.

For which of the following reactions is delta H rxn equal to Delta H formation of the products? THE HEAT OF FORMATION IS DEFINED BY A REACTION THAT FORMS ONE MOLE OF PRODUCT. Thank you. please help

CHE 106 Lecture Notes - Lecture 19: Enthalpy, Joule

CHE 106 Lecture 18: Calorimetry

CHE 106 Lecture Notes - Lecture 19: Enthalpy, Joule

CHE 106 Lecture 20: Lecture 20: Chapter 6: Section 5 -7

Document Summary

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