Apply Henry’s law and Raoult’s law for gases dissolved in liquids.

Explain the The liquid–vapor saturation curve of a pure substance (numerical values are for water).

A 6-kg block of copper at 300 °C is submerged in 0.08 m3 of water at 0 °C contained in an insulated tank. Estimate the final equilibrium temperature. Conservation of energy requires that the energy lost by the copper block is gained by the water. Units are in Celsius.

The expression for the Joule Thompson coefficient for a gas described by the van der Waals equation of state, at low pressures, can be expressed as: 1 2a -—- (2017-b) Cp\R* T i) What will μT be for an ideal gas? Why must this be the case? ii) How does this expression simplify at high temperature? a) Will μT be positive or negative? b) How does temperature change under conditions of low pressure and high temperature, when this gas expands? iii) How does this expression simplify at low temperature? a) Will μT be positive or negative? b) How does temperature change under conditions of low pressure and low temperature, when this gas expands? iv) Calculate the Joule Thompson coefficient of ethane at 300K and 600K. HJT = You can find the heat capacity needed at the NIST Webbook. Search for ethane and then go to the "Gas phase thermochemistry data." Use the values for 1 bar. Pay close attention to units. Your answer should have units of K/atm. The vdw parameters for ethane are: a…