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A: As we know work done is given by: Change in internal energy = heat absorbed + work done
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A: PA = 12.0 atm VA = 10.00 L
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A: Step : 1 Hey since you have posted multiple questions we will answer first question only…
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A: First law of thermodynamics is stated as follows,
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A: Please see the attachment.
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A: GIVEN: Desired Equation : 2N2 + 5O2 → 2N2O5
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A: Extensive property => properties of substance which are depend on mass or amount of substance.…
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A: Determine (e)
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- 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 ΔGA rigid vessel contains 0.014 m3 of saturated-vapor steam in equilibrium with 0.021 m3 of saturated-liquid water at 373.15 K (100°C). Heat is transferred to the vessel until one phase just disappears, and a single-phase remains. Which phase (liquid or vapor) remains, and what are its temperature and pressure? How much heat is transferred in the process?1 kg of benzene is poured into a flask and heated to 353 K (the boiling point of benzeneat 1 atm.) using a heating element that has a power of 700 W (we ignore thatit's probably not so healthy and smart to do). After 5 minutes, when the benzene has stoodboiling point, the heating element is taken up, and the remaining mass of benzene in the flaskmeasured at 470 grams. Determine the enthalpy of vaporization of benzene.
- Find 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.The isothermal compressibility, κT, of lead at 293 K is 2.21 × 10−6 atm−1. Calculate the pressure that must be applied in order to increase its density by 0.10 per cent.Calculate the ΔHsoln and ΔSsoln for the dissolution of solid KHP from the trendline equation of your scatter graph. Include units. Reffer to equation 4. R is the gas constant 8.314J mol-1 K-1 The trendline equation -5623*x + 17.7 Equation 4 Ln Ksp = - ΔHsoln/R (1/T) + ΔSsoln/ R
- What is w when 1.83 kg of H20(1), initially at 25.0 °C, is converted into water vapour at 185 °C against a constant external pressure of 1.00 atm? Assume that the vapour behaves ideally and that the density of liquid water is 1.00 g/ml (Remember to include a+or-sign as appropriate.) Enter your answer in acceptable SI units, accurate to 3. significant figures. Use an acceptable Sl symbol for units.Estimate the density of liquid ethanol at 180°C and 200 bar. Estimate the volume change of vaporization for ammonia at 20°C. At this temperature the vapor pressure of ammonia is 857 kPa.Naphthalene , C10H8, melts at 80.2 oC. If the vapor pressure of the liquid is 1.3 kPa at 85.8 oC and 5.3 kPa at 119.3 oC, use the Clausius-Clapeyron equation to calculate (i) the enthalpy of vaporization, (ii) the normal boiling point, and (iii) the entropy of vaporization at the normal boiling point.
- Naphthalene, C10H8, melts at 80.2 °C. If the vapor pressure of the liquid is 1.3 kPa at 85.8 °C and 5.3 kPa at 119.3 °C, use the Clausius-Clapeyron equation to calculate (i) the enthalpy of vaporization, (ii) the normal boiling point, and (iii) the entropy of vaporization at the boiling point.Consider a container of volume 40.0 dm3 that is divided into two compartments of equal size. In the left compartment there is helium at 1.0 atm and 25C; in the right compartment there is argon at the same temperature and pressure p= 2 atm. What are G, S and H for the process occurring when the partition is removed. Assume that the gases are perfect.Oxygen O2 ,at 200 bar is to be stored in a steelvessel at 20 0 C .The capacity of the vessel is 0.04m3 . Assuming that O2 is a perfect gas .calculate the mass of oxygen that can be stored in the vessel . Thevessel is protected against excessive pressure by a fusible plugwhich will melt if the temperature rises too high .At whattemperature must the plug melt to limit the pressure in the vesselto 240 bar ? .the molar mass of oxygen is 32 Kg/Kmol