For liquid with the typical values a= 0.01 K-1 , K= 0.002 atm 1, Vm= 50 cm/mol, C, p,m = 135 J/mol.K. Calculate C,.m %3D (J/mol.K) at 202 K and 1 atm. O a. 84.00 b. -27220.00 O c. 49.80 O d. -13585.00
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- How much heat (kJ) is required to convert 3.12 moles of liquid benzene at 75.1°C to gaseous benzene at 115.1°C? The following information may be useful.b.p = 80.1CCm (liquid benzene) = 136.0 J/ (mol * °C)ΔHvap = 30.72 kJ/molCm (gaseous benzene) = 36.6 J/ (mol * °C) 102.0 101965 36.8 94.0Calculate the entropy and enthalpy of vaporization for 1 mole of water at room temperature (25oC) and 1 atm from these thermodynamic data:Cm,p(H2O, liquid) = 75.29 J/K·mol, Cm,p(H2O, gas) = 33.58 J/K·mol and ∆vapH(H2O) = 40700 J/ mol (at 100oC)The following information is given for antimony at 1 atm: Tb= 1440.00°C Hvsp=(1440.00°C) = 1.605*10^3 J/g Tm= 631.00°C H fus=(631.00°C) =161.1 J/g Specific heat solid = 0.2090 J/g °C Specific heat liquid = 0.2590 J/g °C A 21.10 g sample of solid antimony is initially at 609.00°C. If the sample is heated at constant pressure ( P= 1 atm), what kJ of heat is needed to raise the temperature of the sample to 729.00°C.
- Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ mol-1. Calculate the value at 153 0C. Given Cp,m for H2O(g): 33.58 kJ mol-1; H2 (g): 28.84 kJ mol-1; O2 (g): 29.37 kJ mol-1. Assume heat capacities are independent of T. NOTE:answer in kilojoules per mole (kJ/mol)Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 791.0 g sample of acetone sitting in the lab has a temperature of 21.7°C. How much heat would be involved in lowering the temperature of the acetone to -200.0°C? (answer in Joules)Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 523.70 g sample of acetone gas has a temperature of 56.0°C. How much heat is involved in converting it to a solid that has a temperature of -94.0°C? (Answer in Joules)
- Substance X has a heat of vaporization of 41.4 kJ/mol at its normal boiling point (423°C). For the process X(l) → X(g) at 1 atm and 423°C calculate the value of ΔSuniv, ΔSsurr, and ΔSsys and ΔGFor 2-methylbutane, the ∆H° of vaporization is 25.22 kJ/mol and the ∆S° of vaporization is 84.48 J/mol･K. At 1.00 atm and 261 K, what is the ∆G° of vaporization for 2-methylbutane, in kJ/mol? give the answer in the right amount of sig figsFind expressions for α and κ for a solid obeying the following equation of state: V = nc1 + nc2P + nc3T + nc4P2 – nc5PT Given that V is volume, P is pressure, T is temperature, n is number of moles, and c1, c2, c3, c4, and c5 are constants.
- Can you help me show the process in this problem? Thermodnamics Suppose that 2.5 mmol Ar(g) occupies 72 dm3 at 298 K and expands to 100 dm3. Calculate ΔG for the process. Ans: -20 kJ1. A certain ideal gas whose R = 278.6 J/kg.K and cp =1.015 kJ/kg.K expands isentropically from 1517 kPa, 288°6 to 965 kPa. For 454 g/s of this gas determine, (a) Wn, (b) V2, (c) ΔU and (d) ΔHWhat is the correct statement about the reaction? (At 298K, ∆H°f for CF4(g) is –933 kJ) ½ C(graphite) + F2(g) → ½ CF4(g) ∆H°rxn > 0 and ∆S°rxn < 0 At high temperatures, ∆G°rxn < 0 For CF4(g), ∆H°rxn = 2 x ∆H°f w > 0