P3C.4 The molar heat capacity of anhydrous potassium hexacyanoferrate(II) varies with temperature as follows: T/K 10 20 30 40 50 60 Cpm/(J K"'mol") 14.43 2.09 36.44 62.55 87.03 111.0 P.m T/K 70 80 90 100 110 150 Cpam/(JK"mol") 131.4 149.4 165.3 179.6 192.8 237.6 P.m' T/K 160 170 180 190 200 Cpam/(JK mol") 247.3 256.5 265.1 273.0 280.3 Determine the Third-Law molar entropy at 200K and at 100 K.

Exercise 7.2.1: Heat from a generic reaction. A balance stoichiometric reaction 2D + 0.5E 3.8F with Ah-(100°C, 1 atm) = -48 kJ/mol. (a) If 62 mol/s of component F are produced at 100°C and 1 atm, how much heat (kW) is produced by the reaction?

A thermocouple lead consists of a small sphere of constantan (a Cu-Ni alloy) having a diameter of 1 mm. Constantan has a density (ρ) of 8920 kg/m3 , a thermal conductivity (k) of 24 W/(m.K), and a heat capacity (Cp) of 410 J/(kg.K). The thermocouple lead is initially at 20 ºC. It is placed into a hot air stream at 200 ºC. The heat transfer coefficient, h between the thermocouple lead and the air is 300 W/(m2 .K). a) Determine which resistance controls the heat transfer process. b) Determine the time required for the thermocouple reading to reach 95% of its total temperature change.***Do not copy from chegg. That one is not correct.

An unfrozen food product has a specific heat of 4 kJ/kg°C and a latent heat of fusion of330 kJ/kg. Once it is frozen its specific heat is 1.98 kJ/kg°C. Its freezing point is -2°C.Determine the total amount of heat (W) to be removed to freeze 100 kg/h of the productfrom an initial temperature of 8°C to -18°C.

Q.3 Two formulas for the heat capacity of CO are given here: C,(cal/(mol-"C)] = 6.890 + 0.0014367(°C) C,(Btu/(lb-mole "F)] = 6.864 + 0.00079787('F) Starting with the first formula, derive the second. (Recall Section 2.5, and remember that the tem- perature unit in the denominator of C, refers to a temperature interval.)

A stream flowing at a rate of 30kgmol/h containing 30% (mole) N₂ and 70% (mole) H₂. This is to be heated from 300 K to 470 K. Calculate the amount of heat transferred using the C data given below. CP N₂ = 29.57 - 5.43 × 10-³T + 13.17 x 10-672, kJ/kgmol -K CHH₂ = 28.65 +1.02 x 10-³T-0.15 x 10-672, kJ/kgmol - K

A CHM student completing the calorimetry experiment mixes 20.0 mL of 1.10 M HCl (aq) with 20.0 mL of 1.05 M NaOH (aq), and observes the temperature increase of 6.611∘∘C.  Assume that the density of each solution is 1.02 g/mL, and the specific heat for the resulting solution is 4.02 J/g∙℃.  Calculate the change in enthalpy for this reaction (ΔHrxn) in kJ/mol H2O.   Use the correct sign (+ or -) and significant figures.

2. Fruit is impeded from ripening when it reaches high temperatures (>32°C). Farmer Joe is roo worried that Princeton's summer heat wave will affect the ripening of his ground cherries. The spherical fruit (1 cm in diameter) is surrounded by a spherical papery husk (husk = 0.3 W/m K) with an inner diameter of 2 cm and an outer diameter of 2.1 cm. The air in between the fruit and the husk is stagnant (air = 0.03 W/m K). On a calm day in July, the Princeton air (outside of the husk) is very warm, with a temperature of ~38°C and a heat transfer coefficient of hPrinceton,calm = 10 W/m².K. (a) Sketch the system, labeling all temperatures, dimensions, and proportionality constants.

What is the final temperature of a 200.00 gram sample of water (c = 4.18 J/g°C) that absorbs 5,000 Joules of heat energy after starting with a temperature of 20°C?

The heat capacity (Cp) of an halogenated organic compound, chloroform is given by the follow equation. Equation (1) Cp (J/mol K) = 19.8 +0.22 T – 0.00026 T² (a) Obtain a new equation that uses T in Fahrenheit (b) Calculate the Cp of chloroform at 300 K using Equation (1) (c) Calculate the Cp of chloroform at 80 °F using the equation you derived in (a)