Oxygen is heated from 700 to 1400 R. Determine the enthalpy energy change Δh of oxygen, in Btu/lbm, using the empirical specific heat equation as a function of temperature from the table. (You must provide an answer before moving on to the next part.) The enthalpy energy change of oxygen is Btu/lbm.
For the given temperature range I have used the variation of specific heat at constant pressure from P.K. Nag Book.
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Oxygen is heated from 700 to 1400 R. Determine the enthalpy energy change Δh of oxygen,...
3. Air is heated from 5400 R to 12000 R while the pressure drops from 50 lbf/in2 to 40 lbf/in2, assuming constant specific heat (Cp 0.24 Btu/lbm-R) and R 53.33 Btu/lbm-R (a) Determine the change of entropy per pound of air (b) If the air was cooled from 1200° R to 540° R while the pressure drops from 50 lbf/in2 to 40lbf/in2 what does it say about the system entropy? Does the result violate the entropy increase principle? 3. Air...
17.55. Use equation 17.56 to determine the change in energy, AE, when 1 mole of Ar is heated from 298 K to 348 K at constant volume. Compare this result with the change in energy calculated using (mass)(specific heat)(change in temperature). The specific heat of argon is 20.79 J/(moly. 17.55. Use equation 17.56 to determine the change in energy, AE, when 1 mole of Ar is heated from 298 K to 348 K at constant volume. Compare this result with...
Determine the hfg of refrigerant-134a at 10°F. Use data from the tables. The gas constant of refrigerant-134a is R = 0.01946 Btu/lbm·R. Consider Clapeyron equation for calculations. (You must provide an answer before moving on to the next part.) The hfg of refrigerant-134a at 10°F is ____ Btu/lbm.
Required information NOTE: This is a multi-part question. Once an answer is submitted, you will be unable to return to this part. The air in a room has a dry-bulb temperature of 75°F and a wet-bulb temperature of 60'F. Assume a pressure of 13 psia. The specific heat at constant pressure is 0.24 Btu/lbm"F. Use data from the tables. Solve using an appropriate software Determine the specific humidity. (You must provide an answer before moving on to the next part.)...
Calculate the change in enthalpy as 1 Kg of nitrogen is heated from 1000 K to 1500 K, assuming the nitrogen is an ideal gas at a constant pressure. The temperature-dependent specific heat of nitrogen is: Cp = 39.06 - 512.79T^-1.5 + 1072.7T^-2 - 820.4T^-3, Cp is in kJ /kmole· K, and T is in K. a) 600 kJ b) 700 kJ c) 900 kJ d) 800 kJ e) 1000 kJ
Oxygen gas is heated in an isobaric process at 177kPa from 49oC to 337oC. Determine the change in specific entropy using (a) the average specific heat and (b) exact values from the appropriate table. Your answers should be very close to each other.
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
A 17-ft3 rigid tank initially contains saturated refrigerant-134a vapor at 160 psia. As a result of heat transfer from the refrigerant, the pressure drops to 50 psia. a.) Determine the final temperature. Use data from refrigerant tables. (Please provide an answer before moving on to the next part.) b.) Determine the amount of refrigerant that has condensed.(lbm) (Please provide an answer before moving on to the next part.) c.) Determine the heat transfer. (Btu)
Part A Calculate the enthalpy change, ΔH, for the process in which 42.4 g of water is converted from liquid at 15.3 ∘C to vapor at 25.0 ∘C . For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and Cs = 4.18 J/(g⋅∘C) for H2O(l). How many grams of ice at -16.2 ∘C can be completely converted to liquid at 25.5 ∘C if the available heat for this process is 4.77×103 kJ ? For ice, use a specific heat of...
Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change q=m⋅Cs⋅ΔT where Cs is specific heat and m is mass. Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase change q=n⋅ΔH where, n is the number of moles and ΔH is the enthalpy of fusion, vaporization, or sublimation. The following table provides the specific heat and enthalpy...