Concept explainers
(a)
Interpretation:
Vapor pressure of acetone at
Concept introduction:
The Clausius-Clapeyron equation is defined as:
Here,
(b)
Interpretation:
Vapor pressure of acetone at
Concept introduction:
Antoine equation is used to determine the vapor pressure of any substance at the given temperature by the equation:
Here,
(c)
Interpretation:
Vapor pressure of acetone at
Concept introduction:
AntoineP is the function in APEx used to calculate the vapor pressure of a pure substance at specific temperature.
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EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- What is AG for the decomposition of CaCO3 at 298 K and a partial pressure of CO2 of 4.00x10-4 bar? CaCO3(s) → CaO(s) + CO2(g) AGrxn (298 K, Pco2 = 0.400 mbar) = ??? CO2(g) Compound AG°; (kJ mol·1) CACO3(s) СаО(s) -1129 -604 -394arrow_forward(c) For reaction 1 taking place at 120 °C: Hg0(s) + S02(g)= Hg(1) + SO3(g) Reaction 1 AreactG® = -13.6 kJ mol-1 %3D (i) Given the standard Gibbs free energy above for reaction 1, calculate AreactG when the partial pressures for S0, and SO2 are 1 bar and 0.004, respectively. (ii) Calculate the equilibrium constant for the reaction and hence state what will be the mole fraction of SO3 in the gas phase at equilibrium. Note: In calculation assume K=÷; where the term x is the mole fraction of SO3. 1-xarrow_forward(b) (i) Mixtures of molten salts often result in high excess mixing enthalpies. Calorimetric experiments of a 25:75 mixture of NaCl and KCl revealed an enthalpy of mixing ΔmixH of -0.4095 kJ mol-1 . Calculate β for this mixture. (ii) Aluminium boils at 2737 K at 100.0 kPa pressure. Given that at 100.0 kPa the molar heat capacity (Cp) of liquid aluminium is 29.30 J K-1 mol-1 , and of aluminium gas is 20.79 J K-1 mol-1 , calculate the total entropy change for the reaction: Al(liquid, 2000 K) → Al (gas, 3500 K). ΔvapS = 49.24 J K-1 mol-1arrow_forward
- 4. The reaction of metallic cobalt (Co) with oxygen can be described by Co(s) + O2 CoO(s) in which the label (s) indicates reactants and products in a solid form. The Gibbs energy change for this reaction at oxygen pressure po, = latm is given by the expression, kJ AG (T) = -500.8- kJ =)T molK mol + (0.164- in which T is the temperature in kelvin. This energy change is per mole of O2 consumed. You might refer to the Ellingham diagram discussed in class and included in the lecture slides to see if the numbers seem to match the plot for that particular reaction. a) Recall that AG = AH - TAS, and that AH and AS only display a weak temperature dependence. Compare to the above equation for AG, What does that tell you about the sign of AS for the reaction? Is it positive or negative? Explain why the sign makes sense for that particular reaction, and also note the slope of this reaction in the Ellingham diagram. Is it consistent? Note that the slopes in the Ellingham diagram relate to the…arrow_forward) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?,co (»= -26.41 kcal/mol, AH9,cH,0H(0)= -48.08 kcal/mol, AG,co ()= -32.8079 kcal/mol, AG?.cH,oH()= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT² + dT³, where C§ is in cal/mol-K and T is in K |Component CH;OH CO b x10 с х105 -0.291 0.1283 a d ×10" 4.55 6.726 2.186 0.04 -0.0457 -1.92 -0.5307 -0.2079 6.952 0.09563arrow_forwardan unknown solid was dissolved in water then precipitated to to get aliquots with decreasing concentrations. the resulting solubility constants of the aliquot were graphed against the inverse of temperature and the equation of the line was y= -5.592.5x +48.33 find the standard enthalpy of the reaction at 30.9 degrees C and report to 2 decimal placesarrow_forward
- In a particular biokgikal reaction taking place in the body at 37 C, the change in enthalpy was -125 kJ mol' and the change in entropy was -126 JK' mol". (a) Cakulate the change in Gibbs energy. (b) Is the reaction spontaneous? (e) Cakulate the total change in entropy of the system and the surroundings.arrow_forward50.0mL of 0.300M CuSO4 is mixed with equal volume of 0.400M. The reaction temperature raised by 3.20oC. a) Determine the molar enthalpy of reaction. 2 NaOH + CuSO4 à Cu(OH)2 + Na2SO4 b) Write a thermochemical equation (with enthalpy value embedded in the equation) to represent the reaction:arrow_forwardThe reduction of iron(III) oxide (Fe,0,) to pure iron during the first step of steelmaking, 2 Fe,0, (s) – - 4 Fe(s) + 30,() is driven by the high-temperature combustion of coke, a purified form of coal: 圖 C(s) + 0,(g) → Co, (g) dlo Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO, and Fe, O, are -428. kJ/mol and -833. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 2000. kg of pure iron. Round your answer to 2 significant digits. Okg Explanation Check O 2021 McGraw-Hill Education. AlI Rights Reserved. Terms of Use| Privacy | Accessibilityarrow_forward
- Hydrogen gas can be produced from the reaction of graphite and steam according to the following reaction: C(s, graphite) + H2O(g) - CO(g) + H2(g) K = 2.77x10-4 at 650 K 2.67 bar of gaseous H20 and excess graphite are added to a sealed container and then heated to 650 K. What is the partial pressure of gaseous H2, in units of bar, when the system reaches dynamic equilibrium?arrow_forwardA mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH3)3CCI) is 3.45 at 500.0 K. (CH3);CCI(g) = (CH3),CCH2(g) + HCI(g) Based on your ICE table, set up the expression for K for the decomposition of (CH3);CCI. (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 Do not combine or simplify terms. K = 3.45 5 RESET (P(CH);CCH;) (P(CH,);CCH,)? (PHCI) (Рнс) (P(CH,),cCi) (P(CH,),CCI)? 2(Рнс) 2(P(CH3),CCH;) 2(P(CH,),CCI) 2(P(CH,),CCI)? 2(Рнс)? 2(P(CH3),C=CH,)?arrow_forward(c) For reaction 1 taking place at 120 °C: Hg0(s) + S02(g) = Hg(l) + S03(g) Reaction 1 AreactG = -13.6 kJ mol-1 (i) Given the standard Gibbs free energy above for reaction 1, calculate AreactG when the partial pressures for S0, and SO2 are 1 bar and 0.004, respectively. (ii) Calculate the equilibrium constant for the reaction and hence state what will be the mole fraction of SO3 in the gas phase at equilibrium. Note: In calculation assume K=÷; where the term x is the mole fraction of SO3. 1-xarrow_forward
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