The dissolving process of a particular salt is an endothermic process, but it leads to an increase in entropy. After studying the solubility of the salt at different temperatures, it was found that the solubility decreases as temperature decreases. Using concepts like entropy and Gibb's energy, explain why the solubility of the salt decreases as the temperature of water decreases.

Determine the equilibrium vapor pressure of germanium metal at 326.0 °C. The standard enthalpy of vaporization of germanium is 376.6 kJ/mol and the vapor pressure at 100.0 °C is 1.6E-32 Pa.

A reaction has a standard free‑energy change of −18.20 kJ (−4.350 kcal mol−1). Calculate the equilibrium constant for the reaction at 25 °C.   Keq =

Most of the coal available in the United States is bituminous or "soft" coal, which contains as much as 5% sulfur by weight. When this coal is burned, the sulfur reacts with oxygen to form sulfur dioxide gas. When the sulfur dioxide gas dissolves in raindrops, it forms sulfuric acid. This is how we get acid rain. Here is the reaction that produces sulfur dioxide gas when soft coal is burned: S,()+80, (g) - 880,(g) Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 153.9 g of solid sulfur and 27.1g of oxygen gas each. The volume and temperature of each vessel is shown in the table below. db Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. initial rate of vessel volume…

A student dissolves 11.0 g of ammonium chloride (NH, CI) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 20.0 °C to 16.8 °C over the course of 6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH,CI(s) NH (aq) + Cl (aq) db You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ kJ…

A student dissolves 12.3 g of potassium chloride (KCI)in 250. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0 °C to 19.6 °C over the course of 5.9 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: olo Ar KCI(s) K* (aq) + CI (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. exothermic Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. |kJ kJ Calculate…

How many Calories should there be in three grams of pure sucrose?A.4B. 12C. 18D. 8E. None of the above.

For a certain chemical reaction, the standard Gibbs free energy of reaction at 5.00 °C is -76.7 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 ☐ x10 × Ś

You add some of the white crystals to a small test tube filled with water. The water in the test tube was initially at room temperature (25˚C). Once the crystals were added and the tube was stirred, the temperature of the solution decreased to about 15˚C and all of the crystals dissolved. what is the change in Gibbs free energy (∆G) for this process?