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CH 301 Midterm: thermodynamics study guide

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pearsea-lion802

30 Nov 2016

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Th er mo dy na mi cs test review state functions are properties that are path dependent. Extensive properties change with amount of substance. Intensive properties do not change with amount of substance first law of thermodynamics states that energy is neither created nor destroyed, only changed in form. Where w can equal -p v (1 latm = 101. 325 j) or - nrt. +w: surroundings do work on the system. +q: absorbed heat equipartition theorem: each particle contributes to u by kt for each mode. (3)rt enthalpy: heat flow at constant pressure between systems and surroundings. H vap is huge because you have to break all imfs to vaporize. Standard conditions are 1 molar concentration, 298k, 1 atm. Bond energies: amount of energy required to break 1 mole of bond. Q = nrtln(v 2 /v 1 ) calorimetry: measuring q output. To convert: u = h - nrt.

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Related Questions

Energy cannot be created nor destroyed, but it can be transferred between a reaction and its surroundings. The change in energy, Delta E, is positive if the reaction absorbs energy, and it is negative if the reaction releases energy. You may also see this expressed in terms of change in internal energy, Delta U. For the purposes of this question, Delta U and Delta E are equal. One way a reaction can transfer energy to or from the surroundings is by releasing or absorbing heat. A reaction can also transfer energy, in the form of work, through a change in volume. The total change in energy is the sum of the heat and work: Delta E = q + w At constant pressure, q = Delta H and w = -P Delta V and so Delta E = Delta H - P Delta V Assuming constant pressure, rank these reactions from most energy released by the system to most energy absorbed by the system, based on the following descriptions: Surroundings get colder and the system decreases in volume. Surroundings get hotter and the system expands in volume. Surroundings get hotter and the system decreases in volume. Surroundings get hotter and the system does not change in volume. Also assume that the magnitude of the volume and temperature changes are similar among the reactions. Rank from most energy released to most energy absorbed. To rank items as equivalent, overlap them. Energy cannot be created nor destroyed, but it can be transferred between a reaction and its surroundings. The change in energy, Delta E, is positive if the reaction absorbs energy, and it is negative if the reaction releases energy. You may also see this expressed in terms of change in internal energy, Delta U. For the purposes of this question, Delta U and Delta E are equal. One way a reaction can transfer energy to or from the surroundings is by releasing or absorbing heat. A reaction can also transfer energy, in the form of work, through a change in volume. The total change in energy is the sum of the heat and work: Delta E = q + w At constant pressure, q = Delta H and w = -P Delta V and so Delta E = Delta H - P Delta V A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g) + 4Y(g) - 2Z(g), Delta H degree = -75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L Calculate the value of the total energy change. AE, in kilojoules. Express your answer with the appropriate units.

At constant pressure, the combustion of 10.0 g of C2Hg(g) releases 518 kJ of heat. What is AH for the reaction given below? 2 C2H6(g) +- 7 O2(g) rightarrow 4 CO2(g) + 6 H2O(l). -779 kJ -1560 kJ -86.1 kJ -3120 kJ Use the information provided to determine Delta H degree r times n for the following reaction: CH4(g) + 3 Cl2(g) rightarrow CHCI3(I) + 3 HCI(g) Delta H degree r times n = ? -217 kJ -335 kJ +662 kJ +117 kJ -151 kJ Choose the reaction that illustrates Delta H degree f for NaHCO3. Na(s) + 2 H(g) + C(s) + 3 O(g) rightarrow NaHCO3 (s) Na(s) + H2(g) + C(s) + O2(g) rightarrow NaHCO3 (s) Na+(aq) + H2O (I) + CO2 (g) rightarrow NaHCO3 (s) Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) rightarrow NaHCO3 (s) Na+(aq) + HCO3 -1 (aq) rightarrow NaHCO3 (s) Use the standard reaction enthalpies given below to determine Delta H degree r times n for the following reaction: 4 SO3(g) rightarrow 4 S(s) + 6 O2(g) Delta H degree r times n = ? Given: SO2(g) rightarrow S(s) + O2(g) Delta H degree r times m = +296.8 kJ 2 SO2(g) + O2(g) rightarow 2 SO3(g) Delta H degree r times n = -197.8 kJ -494.6 kJ -791.4 kJ 1583 kJ -293.0 kJ -692.4 kJ Which of the following statements is TRUE? State functions do not depend on the path taken to arrive at a particular state. Energy is neither created nor destroyed, excluding nuclear reactions. Delta Hr times r can be determined using constant pressure calorimetry. Delta H r times n can be determined using constant volume calorimetry. All of the above are true. How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) rightarrow Al2O3(s) + 2 Fe(s) Delta H degree r times n = 852 kJ 01.51 times 103 kJ 241 kJ 0482 kJ 4.20 x 103 kJ 753 kJ Given w = 0, an endothermic reaction has the following. - Delta H and + Delta E Delta H and -Delta E - Delta H and -Delta E + Delta H and +Delta E Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat? 10.0 g ethanol, Celharol = 2.42 J/g degree C 10.0 g Ag, CAg = 0.235 J/g degree C 10.0 g Au, CAu = 0.128 J/g degree C 10.0 g Fe, CFe = 0.449 J/g degree C 10.0 g H2O, CHO = 4.18J/g degree C Which of the following processes is endothermic? a hot cup of coffee (system) cools on a countertop the vaporization of rubbing alcohol the chemical reaction in a "hot pack" often used to treat sore muscles the freezing of water the combustion of propane

Show transcribed image text At constant pressure, the combustion of 10.0 g of C2Hg(g) releases 518 kJ of heat. What is AH for the reaction given below? 2 C2H6(g) +- 7 O2(g) rightarrow 4 CO2(g) + 6 H2O(l). -779 kJ -1560 kJ -86.1 kJ -3120 kJ Use the information provided to determine Delta H degree r times n for the following reaction: CH4(g) + 3 Cl2(g) rightarrow CHCI3(I) + 3 HCI(g) Delta H degree r times n = ? -217 kJ -335 kJ +662 kJ +117 kJ -151 kJ Choose the reaction that illustrates Delta H degree f for NaHCO3. Na(s) + 2 H(g) + C(s) + 3 O(g) rightarrow NaHCO3 (s) Na(s) + H2(g) + C(s) + O2(g) rightarrow NaHCO3 (s) Na+(aq) + H2O (I) + CO2 (g) rightarrow NaHCO3 (s) Na(s) + 1/2 H2(g) + C(s) + 3/2 O2(g) rightarrow NaHCO3 (s) Na+(aq) + HCO3 -1 (aq) rightarrow NaHCO3 (s) Use the standard reaction enthalpies given below to determine Delta H degree r times n for the following reaction: 4 SO3(g) rightarrow 4 S(s) + 6 O2(g) Delta H degree r times n = ? Given: SO2(g) rightarrow S(s) + O2(g) Delta H degree r times m = +296.8 kJ 2 SO2(g) + O2(g) rightarow 2 SO3(g) Delta H degree r times n = -197.8 kJ -494.6 kJ -791.4 kJ 1583 kJ -293.0 kJ -692.4 kJ Which of the following statements is TRUE? State functions do not depend on the path taken to arrive at a particular state. Energy is neither created nor destroyed, excluding nuclear reactions. Delta Hr times r can be determined using constant pressure calorimetry. Delta H r times n can be determined using constant volume calorimetry. All of the above are true. How much energy is evolved during the formation of 98.7 g of Fe, according to the reaction below? Fe2O3(s) + 2 Al(s) rightarrow Al2O3(s) + 2 Fe(s) Delta H degree r times n = 852 kJ 01.51 times 103 kJ 241 kJ 0482 kJ 4.20 x 103 kJ 753 kJ Given w = 0, an endothermic reaction has the following. - Delta H and + Delta E Delta H and -Delta E - Delta H and -Delta E + Delta H and +Delta E Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat? 10.0 g ethanol, Celharol = 2.42 J/g degree C 10.0 g Ag, CAg = 0.235 J/g degree C 10.0 g Au, CAu = 0.128 J/g degree C 10.0 g Fe, CFe = 0.449 J/g degree C 10.0 g H2O, CHO = 4.18J/g degree C Which of the following processes is endothermic? a hot cup of coffee (system) cools on a countertop the vaporization of rubbing alcohol the chemical reaction in a "hot pack" often used to treat sore muscles the freezing of water the combustion of propane