Q: Why do the collisions between molecules do not appear in the derivation of the ideal gas law?
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Q: Veritasium (Vr) boils at 30.3°C and its enthalpy of vapourization is 67.3 kJ mol-1. Calculate ΔSsys…
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Q: For an ideal gas of constant volume, what happens to the pressure if the temperature is doubled?
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Q: When heat Q is supplied to a diatomic gas of rigid molecules, at constant volume its temperature…
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Q: For a given species, see the thermodynariic values below. Boiling Point: 80.0° C Melting Point: 10.0…
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Q: One might think that the internal energy of diatomic gases is given by Eint = 5RT/2. Do diatomic…
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Q: Are the Temperature and internal energy state variables? How?
A: Yes, the internal energy and temperature are the state variables.
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A: The solution is given below
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Q: Is it possible to increase the temperature of a gas without adding heat to it? If so how?
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Q: Calculate the specific heat CV of a gas whose diatomic molecules have transition, rotation and…
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Q: Find the total heat capacity at constant pressure of 2.35 mol of an ideal diatomic gas where the…
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Q: An SUV tire contains 0.037 m3 of air at a gauge pressure of 2.61 × 105 N/m2. The composition of air…
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Q: When heat Q is supplied to a diatomic gas of rigid molecules, at constant volume its temperature…
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Q: A monoatomic, ideal gas with volume 5 L and pressure of 6 ATM expands isobarically to a volume of 25…
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Why (in both
The heat capacity is given by
Using the second law of thermodynamics, the entropy is given by
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- Why are there two specific heats for gases Cp and Cv , yet only one given for solid?Q1) The molar specific heat of a diatomic gas is measured at constant volume and found to be 29.1 J/mol. K. The types of energy that arecontributing to the molar specific heat are: (a) translation only (b) translation and rotation only (c) translation and vibration only (d) translation, rotation, and vibration. And why?Below 0.3 K the slope of the 3He solid-liquid phase boundary is negative Use the third law of thermodynamics to argue that the slope of the phase boundary must go to zero at T = O. (Note that the 4He solid-liquid phase boundary is essentially horizontal below 1 K.)
- A 2 mol sample of a diatomic ideal gas (y=1.4) expands slowly and adiabatically from a pressure of 18 atm and a volume of 8 L to a final volume of 18 L. What is the final temprature (in K) of the gas? ( Answer no decimal )scientist wants to do this experiment but modifies it by filling the balloon with 0.66 moles of neon gas, which behaves as an ideal gas. If the balloon initially holds 0.4 L of the gas and expands to 1.7 L after being heated in the pot over the stove, how much work is done by the system if the experiment is performed at 273 K?”Calculate AS when 3.2 moles of n-hexane goes from 298 K and 1 atm to 398 K and 2 atm. The table below provides useful data, all at 298 K and 1 atm (reference: Cerdeiriña, Claudio A., et al. "Isobaric thermal expansivity and thermophysical characterization of liquids and liquid mixtures." Physical Chemistry Chemical Physics 3.23 (2001): 5230-5236). You may neglect the pressure and temperature dependence of all quantities. Compound Molar Volume (cm³/mol) Isothermal Compressibility (1/atm) Thermal Expansity (1/K) Cp,m (J/molK) n-hexane 133.09 1.69 x 10-4 1.38 x 10-3 195.66 n-heptane 147.45 1.47 x 10-4 1.246 x 10-3 224.64 n-dodecane 228.55 1.00 x 10-4 9.69 x 10-4 376.22
- The derivation of the ideal-gas equation included the assumption that the number of molecules is very large, so that we could compute the average force due to many collisions. However, the ideal-gas equation holds accurately only at low pressures, where the molecules are few and far between. Is this inconsistent? Why or why not?An SUV tire contains 0.037 m3 of air at a gauge pressure of 2.61 × 105 N/m2. The composition of air is about 78% nitrogen (N2) and 21% oxygen (O2), both diatomic molecules. How much more internal energy, in joules, does the air in the tire have than the same volume of air has at zero gauge pressure outside the tire? Einternal,2−Einternal,1 = ? Hints: -Assume not only equal volumes but also equal temperatures.-Since the temperature is constant, what must be changing in this process?-The heat capacity, and thus the internal energy, depends upon whether gas is monatomic or diatomic.A car tire contains 0.0440 m3 of air at a pressure of 2.75 x 10° N/m2 (about 40 psi). How much more internal energy (in J) does this gas have than the same volume has at zero gauge pressure (which is equivalent to normal atmospheric pressure)? (Assume the tire pressure of 2.75 x 105 N/m2 is absolute pressure, not gauge pressure. Assume for this question that air is monatomic.) Additional Materials O Reading Submit Answer
- Find the correct statements about the Clausius-Clapeyron equation. (1) (111) The boiling point of liquid raises with increase in pressure when the change in specific volume (V₂-V) is a negative quantity. The melting point of the ice is lowered with increase in pressure when the change in specific volume (V₂-V) is a negative quantity. The Clausius-Clapeyron equation is derived from thermodynamic relation ap ¹(37), - (), (iv) The Clausius-Clapeyron equation failed to explain the phenomena of regelation of ice. (a) (i), (ii), and (iii). (b) (i) and (iv) (c) (ii) and (iii) (d) (i) and (iv)The molar specific heat at constant pressure of an ideal gas is (7/2)R. The ratio of specific heat at constant pressure to that at constant volume is (a) 7/5 (b) 8/7 (c) 5/7 (d) 9/7In an industrial process, a fuel-air mixture is fitted with a piston. When the mixture is ignited at a constant pressure of 700mm Hg, 2.0 kJ of energy is released and is found to occupy a final volume of 200L. What would be the initial volume occupied by the mixture if all energy released is converted as work done by the system to push the piston?