Suppose 2.00 mol of an ideal gas is contained in a heat-insulated cylinder with a moveable frictionless piston.Initially, the gas is at 1.00 atm and 0°C. The gas is com-pressed reversibly to 2.00 atm. The molar heat capacity atconstant pressure, c, equals 29.3 J K-1 mol¯!. Calculatethe final temperature of the gas, the change in its internalcncrgy, AU, and the work done on thegas.

Given data: Moles of gas (n) = 2 Pressure of gas (P1) = 1 atm Pressure of gas (P2) = 2 atm Molar…

Answered: Suppose 2.00 mol of an ideal gas is…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 58P

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A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
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.
Use the heat capacities of the products and reactants of the thermite reaction and the calculated H of the process to estimate the temperature of the reaction. Assume that all of the heat generated goes to increasing the temperature of the system.
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What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?
If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is CT- = 56.990.1202T J/mol.K, how much heat is needed?
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To properly determine the internal energy of combustion methylhydrazine, the calorimeter was first calibrated. A 0.4500 g sample of sucrose (MW 342.296 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.98 K. For sucrose, the internal energy combustion at constant volume, ∆U, is known to be –5616.64 kJ/mol. Calculate the calorimeter constant, in kJ/K.
An oxyacetylene flame is often used in the welding of metals. Estimate the flame temperature produced by the reaction 2C2H2 (?) + 5O2 (?) ⟶ 4CO2 (?) + 2H2O(?) a) Using appropriate tabulated data (heats of formation) determine the heat of reaction at 298K. b) Now assume this reaction occurs at 2270K. Estimate the approximate enthalpy at the higher temperature using the heat capacities of these substances.
a sample of 98g of pure sulfuric acid is dissolved in 2.0 kg of water in an insulated vessel at 15°C, and thetemperature rises rapidly because of the process of forming the solution. The reaction is summarized in theequation H2SO4(l) -> H+(aq) + HSO4 –(aq). Estimate the temperature change assuming that the heat capacityof the solution is 4.0 J/gK and the heat capacity of the vessel is 300 J/K.
1.5-mol ideal gas initially at 220 K is compressed reversibly and adiabatically from 45.0 L to 15.0 L. The molar heat capacity at constant volume for this gas is Cv,m = 5R/2 and is independent of temperature. The work of this process should be equal to _________ Kilo-Joule with the correct sign (3 significant figures).
a) A 1.60 dm3 sample of a mixture of methane gas, CH4 and oxygen gas, measured at 25 oC and 101 kPa, was allowed to react in a bomb calorimeter in which, had a heat capacity of 5.30 kJ/K altogether with its contents. The complete combustion of the methane gas to carbon dioxide gas and water caused a temperature rise in the calorimeter of 6.28 K. Given that ∆Ho c (CH4) is -560 kJ/mol. i. Define the standard enthalpy of combustion of methane ii. Write a thermochemical equation for the combustion of methane iii. Knowing the ∆Ho c of methane, calculate the number of mole of methane in the mixture. iv. Calculate the total moles of gases in the calorimeter.

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