2. The graph below represents the chemical potential of a pure substance as a function of the temperature at constant pressure. Solid a) Give the thermodynamic condition so that it occurs a phase transition. Respond using a mathematical expression. Liquid Gas b) Calculate the pressure at which the water would boil at 300 K. ApĦwater) = 40.7 k) / mol. Solid stable Liquid Gas stable stable T, Temperature, T T. Chemical potential, u

2. The graph below represents the chemical potential of a pure substance as a function of the temperature at constant pressure. Solid a) Give the thermodynamic condition so that it occurs a phase transition. Respond using a mathematical expression. Liquid Gas b) Calculate the pressure at which the water would boil at 300 K. ApĦwater) = 40.7 k) / mol. Solid stable Liquid Gas stable stable T, Temperature, T T. Chemical potential, u

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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. 1a. Assume the density and specific heat of water is 1.00 g/mL and 4.184 J/g °C, respectively. Using the data above, determine the for ammonium nitrate in water. Assume the heat capacity of the calorimeter is negligible.
3. Maximum solubility of an ionic compounds in water depend on different sets of conditions. Out of five sets of conditions (given below), which one is the best for getting maximum solubility? A. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be large. B. The enthalpy of hydration (Delta H) of the cation should be equal to the enthalpy of hydration of the anion, regardless of the magnitude of the lattice energy C. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be small. D. The magnitude of the lattice energy should be small, and the enthalpy of hydration of the ions should be large. E. The magnitude of the lattice energy should be large, and the enthalpy of hydration of the ions should be small.
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
Calculate the enthalpy of vaporization of SO2 at –25°C if the same at its boiling point (i.e. –10°C) be 5950 cal mol–1. Given for SO2, molar heat capacities in liquid and vapor phase are 206 cal K–1 mol–1 and 9.3 cal K–1 mol–1 respectively.
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From the following vapor pressure data for ethyl amine, an estimate of the molar heat of vaporization of C₂H5NH₂ is | kJ/mol. P, mm Hg T, K 40.0 233 100. 248
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From your data in Part 1 of the experiment, you calculate the natural log of the partial pressure of water and 1/T value in K for 5 points between 50°C and 80°C. You make a graph of In(P) vs. 1/T and determine that the slope of the linear line is -4800 K. Use this information to calculate AHvap of water. Make sure to use R = 8.314 J mol-1-K-1. Oa. 46.6 kJ/mol Ob. 0.578 kJ/mol Oc. 31.5 kJ/mol O d. 39.9 kJ/mol
One of the most recognizable corrosion reactions is the rusting of iron. Rust is caused by iron reacting with oxygen gas in the presence of water to create an oxide layer. Iron can form several different oxides, each having its own unique color. Red rust is caused by the formation of iron(III) oxide trihydrate. Fe,O, • 3 H,O Write the balanced reaction for the formation of Fe, O, • 3 H,O(s). Phases are optional. reaction: Fe + 6H,O + 30, Fe(OH)3 > Incorrect