1.2Consider a 2.00 mol sample of perfect gas initially at p = 112 kPa and T = 278 K. The temperature ofperfect gas with constant volume heat capacity 3R/2 is reduced by 28 K. Calculate1.2.1 the final pressure. Use 4 significant figures.1.2.2 the change in internal energy. Use 5 significant figures.1.2.3 the heat transferred in the process. Use 5 significant figures.1.2.4 the work done.

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Answered: 1.2 Consider a 2.00 mol sample of…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 87QRT

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In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
The distance between downtown San Francisco and downtown Oakland is 9 miles. However, a car driving between the two points travels 12.3miles. Of these distances, which one is analogous to a state function? Why?
In a constant-pressure calorimeter that is, one that expands or contracts if the volume of the system changes, 0.145 mole of an ideal gas contracts slowly from 5.00 L to 3.92 L. If the initial temperature of the gas is 0.0 C, calculate the U and w for the process.
On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm (STP) evolves 75.65 kJ of heat. If the gas is a mixture of ethane (C2H6) and propane (C3H8), what is the mole fraction of ethane in the mixture?
Calculate the specific heat of a material if 288J of energy were required to heat 50.5g of the material from 298K to 330K. What are the units?
Use the two appropriate values of R to determine a conversion between L. atm and J.
Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.
Liquid hydrogen fluoride, liquid water,and liquid ammonia all have relatively high specific heats for suchsmall molecules. Speculate asto whythis might be so.
Chlorine trifluoride is a toxic, intensely reactive gas. It was used in World War II to make incendiary bombs. It reacts with ammonia and forms nitrogen, chlorine, and hydrogen fluoride gases. When two moles of chlorine trifluoride react, 1196 kJ of heat are evolved. (a) Write a thermochemical equation for the reaction. (b) What is Hf for ClF3?
5. Hydrogen gas burning in excess from oxygen gas in H2g + 1002g → H2O+ excess O2g 298K The heat of vaporization water (-242.44kJ), the heat capacity at pressure constant Gas H2 O2 H2O | C, JK´ mol- Calculate a. AE in 298K 27.17 27.17 31.35 b. AH in 498K

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