lgs everything else). e system (the part you are studyml (reaut nsi ost systems we are interested in will have a constant pressure, mean ing that q (heat or thermal energy) would be equivalent to the change in enthalpy (AH) We defined environments in which heat goes into the system surroundings get hot as exothermic ΔΗ- and the surroundings get cold as EX rmic AH + while environments in which heat goes out of the system and the For each of the environments below: (1) identify your system and surroundings and (2) predict whether it would be endothermic or exothermic. 1. a. Wood burning b. Water freezing c. Sweat evaporating d. Chemical hand-warmer

lgs everything else). e system (the part you are studyml (reaut nsi ost systems we are interested in will have a constant pressure, mean ing that q (heat or thermal energy) would be equivalent to the change in enthalpy (AH) We defined environments in which heat goes into the system surroundings get hot as exothermic ΔΗ- and the surroundings get cold as EX rmic AH + while environments in which heat goes out of the system and the For each of the environments below: (1) identify your system and surroundings and (2) predict whether it would be endothermic or exothermic. 1. a. Wood burning b. Water freezing c. Sweat evaporating d. Chemical hand-warmer

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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Thermochemistry is a branch of chemistry that qualitatively and quantitatively describes the energy changes that occur during chemical reactions. AH(T.) Products AH"(T) Reactants T, Temperature, T (i) Which Law of Thermochemistry is illustrated in the graph above (ii) Accurately define this Law with aid of appropriate equation/s. Enthalpy, H
Using Hess law, compute the thermochemical equation to know the total heat of RXN. C,H. (g) + H2 (g) → C,H« (g) AH = ? C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H¿O (I) C>Ho (g) + 3 ½ 0; (g) → 2 CO2 (g) + 3 H;O (1I) H2 (g) + ½ O> (g) → H;O (1). AH-- 1411.0 kJ AH = -1560.0 kJ AH = -285,8 kJ a. -3216.8 kJ b. -136.8 kJ c. 3216 kJ d. -136.8 J
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8
(c) Consider the following chemical reaction: C;Hs(g) + H2(g) C2H6(g) + CH4(g) ΔΗ? %3D Calculate the enthalpy change for the reaction above using Hess's law. Thermochemical dat: H:(g) + ½O2(g) H2O(1) AH° =-285.8 kJ AH°combustion for CH4(g) AH° =-890.0 kJ/mol %3D CO:(g) C(s. graphite) + O:(g) AH° = +393.5 kJ AH°combustion for C2H6(g) AH = -1560.0 kJ/mol AH°, for C3H$(g) AH° =-103.8 kJ/mol
(D 263 kJ/mol P. 22. Using the following thermochemical equations: C(s) + O,(g) → CO,(g) ΔΗΟ. rxn 1 =-394 kJ/mol,Txn C(s) + CO,(g) → 2 CO(g) AH°. Ixn 2 =+173 kJ/mol,xa Determine the enthalpy of the reaction represented below: 2 C(s) + 0,(g) → 2 CO(g) ΔΗ Txn 3 = ? 1> (A) ΔΗ. :-567 kJ/molxn rxn (В) ДН =-221 kJ/mol,xn (С) ДН =+221 kJ/molpxn (D) AH°. +567 kJ/molpxn %3D Ixn qt ian od geind hw qua boalunai na cop d ofiosa orb d A 100--32 HO0-02 X convinn or rmrainn an nart of this nanA iR llanal.
Measurements show that the energy of a mixture of gaseous reactants increases by 388. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that-88. kl of work is done on the mixture during the reaction. th Calculate the change in enthalpy of the gas macture during the reaction. Round your anawer to 3 significant digits. O exothermic Is the reaction exothermic or endothermic O endothermic
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Using the information provided along with an understanding of Hess's Law, determine the enthalpy of reaction for the unknown reaction. AFels) + 3Sn0,(s) → 2Fe,0,(s) +3Sn(s) 2Fe(s) +0, (s) - Fe;0,(s) A,H = -824.2 k) Sn{s) + 0,(g) - Sn02(s) AyH=-580.7 k/
Calculate AE and determine whether the process is endothermic or exothermic for the following cases: (1) q = 0.123 kJ and w = - 230 J (2) A system releases 66.1 kJ of heat to its surroundings while the surroundings to 44.0 kJ of work on the system.
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Sulfur dioxide, SO, (g), can react with oxygen to produce sulfur trioxide, SO, (g), by the reaction 2 SO, (g) + 0,(g) → 2 SO,(g) The standard enthalpies of formation for SO,(g) and SO, (g) are AH; [SO,() = -296.8 kJ/mol AH; SO,( = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 4.10 L of SO, (g) is converted to 4.10 L of SO, (g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal gas behavior. kJ AL = 18.249 incbrcect