The enthalpy of vaporization of a certain liquid is found to be 14.4 kJ mol−1 at 180 K, its normal boiling point. The molar volumes of the liquid and the vapour at the boiling point are 115 cm3 mol−1 and 14.5 dm3 mol−1, respectively. (a) Use the Clapeyron equation to estimate dp/dT at the normal boiling point. (b) If the Clausius–Clapeyron equation is used instead to estimate dp/dT, what is the percentage error in the resulting value of dp/dT?

A sample of water vapour at 200 C is compressed isothermally from 302c * m ^ 3 to 58c * m ^ 3 What is the change in its molar Gibbs energy?

Assume you are interested in exploring the use of ammonium nitrate (NH4NO3) as the active ingredient in an inexpensive home-made cold pack. You decide that a practical cold pack should be able to depress the temperature of 1 kg of human muscle tissue by 5 oC. Now you need to know the amount of NH4NO3 required to achieve this. Ammonium nitrate is a highly water soluble solid. You believe the enthalpy of dissolution  for NH4NO3 must be determined. To this end, you add 2.339 g of NH4NO3 to 99.7 mL of water at 23.7 °C in a constant-pressure calorimeter and close the calorimeter. The temperature of the water decreases to a minimum of 21.9 °C 1) The specific heat of human muscle tissue (smuscle) is 3.47 kJ/kg oC. Given this value, how many grams of ammonium nitrate (NH4NO3) is required to depress the temperature of 1.00 kg of human muscle by 5.00 oC? Please remember, show all work in a legible, highly organized manner

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One of the more commonly used compressed gases is nitrogen (N2), often in large metal cylinders. If a cylinder holds 711 mol of N2 when pressurised to 5.3 x 104 kPa at T = 20oC, how many litres is its capacity?

The reduction of iron(III) oxide (Fe₂O,) to pure iron during the first step of steelmaking, 2 Fe₂O₂ (s) 4Fe(s) + 30₂ (g) 1 is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + O₂(g) CO₂ (g) - Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO₂ and Fe₂O, are-443. kl/mol and -801. kJ/mol, respectively. Calculate the maximum mass of pure iron that can be produced by the combustion of 8200. kg of coke. Round your answer to 2 significant digits. 0.8 X ?

It is well known that the temperature at which water freezes to ice or boils at a pressure of 1 atm, are 0°C and 100°C. In the next two tasks, we will now investigate what the temperatures would be at the top of Mount Everest, where the pressure is only 0.337 bar. The standard molar enthalpy of fusion of water at 0°C is ΔfusHmo = 6.008 kJ mol-1 and the standard molar enthalpy of vaporization of water at 100°C is ΔvapHmo = 40.656 kJ mol-1. The density of liquid water at 0°C is ρ(l) = 999.9 kg m-3, while the density of ice at 0°C is only ρ(s) = 916.2 kg m-3. The densities and enthalpies are assumed to be independent of temperature. 1) Calculate the temperature at which ice melts on top of Mount Everest. 2) Calculate the temperature at which water boils on top of Mount Everest.

Suppose now that argon is added to the mixture in the previous exercise to bring the composition closer to real air, with mole fractions 0.780. 0.210, and 0.0096, respectively. (a) What is the additional change in molar Gibbs energy and entropy at 298 K? (b) Is the mixing spontaneous?