Problem 55
Estimate the enthalpy of reaction \(\bar{h}_{R}\) for the combustion process of carbon monoxide at \(3960 \mathrm{R}\), using (a) enthalpy data and (b) \(K_{p}\) data.
Problem 57
Estimate the enthalpy of reaction \(\bar{h}_{R}\) for the dissociation process \(\mathrm{CO}_{2} \rightleftharpoons \mathrm{CO}+\frac{1}{2} \mathrm{O}_{2}\) at \(2200 \mathrm{K},\) using \((a)\) enthalpy data and \((b) K_{P}\) data.
Problem 58
Estimate the enthalpy of reaction for the equilibrium reaction \(\mathrm{CH}_{4}+2 \mathrm{O}_{2} \rightleftharpoons \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) at \(2500 \mathrm{K}\), using \((a)\) enthalpy data and \((b) K_{P}\) data. Obtain enthalpy and entropy properties from EES.
Problem 59
Consider a tank that contains a saturated liquid vapor mixture of water in equilibrium. Some vapor is now allowed to escape the tank at constant temperature and pressure. Will this disturb the phase equilibrium and cause some of the liquid to evaporate?
Problem 60
Consider a two-phase mixture of ammonia and water in equilibrium. Can this mixture exist in two phases at the same temperature but at a different pressure?
Problem 61
Using the solubility data of a solid in a specified liquid, explain how you would determine the mole fraction of the solid in the liquid at the interface at a specified temperature.
Problem 62
Using solubility data of a gas in a solid, explain how you would determine the molar concentration of the gas in the solid at the solid-gas interface at a specified temperature.
Problem 65
Water is sprayed into air at \(80^{\circ} \mathrm{F}\) and 14.3 psia, and the falling water droplets are collected in a container on the floor. Determine the mass and mole fractions of air dissolved in the water.
Problem 67
Show that a mixture of saturated liquid water and saturated water vapor at \(300 \mathrm{kPa}\) satisfies the criterion for phase equilibrium.
Problem 68
A liquid-vapor mixture of refrigerant-134a is at \(280 \mathrm{kPa}\) with a quality of 70 percent. Determine the value of the Gibbs function, in \(\mathrm{kJ} / \mathrm{kg},\) when the two phases are in equilibrium.
