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- What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?Show that = T/p for an ideal gas.
- Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.Calculate the molar heat capacity at constant pressure (Cp) for a diatomic H2 gas(y = 1.41) with molar heat capacity at constant volume (Cv) of 20.42 J/mol-K?It has been experimentally determined that the heat of combustion of benzene at constant volume is: ΔU ° rxn = -3265.6 kj, at 298K and the heat of combustion at constant pressure is: ΔH ° rxn = -3261.9 kj. C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l) If we consider that substances in the gas phase behave as ideal gases, responding as appropriate: i) Does the system experience expansion or compression? justify mathematically.
- Calculate the work of expansion accompanying the complete combustion of 10.0 g of sucrose (C12H22O11) to carbon dioxide and (a) liquid water, (b) water vapour at 20 °c when the external pressure is 1.20 atm.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.Physical chemistry - please refer to pics Now, consider 2.0 moles of methane (CH4 ), initially at 273 K, that is reversibly and adiabatically compressed from an initial volume of 10.00 L to a final volume of 2.00 L. 3a. Determine the final temperature, considering the gas to be described by the ideal gas equation of state. 3b. Determine the work required w, the associated heat flow q, and the internal energy change ∆U for the gas between the initial and final states.
- A sample of solid biphenyl weighing 0.5260 g was ignited in a bomb calorimeter initially at 25.0°C, producing a temperature rise of 1.910 K. Determine the internal energy (∆U) of combustion. To properly determine the internal energy of combustion for the solid biphenyl, the calorimeter was first calibrated. a)A 0.7750 g sample of benzoic acid (C₆H₅COOH, MW 122.1 g/mol)) was ignited under identical conditions and produced a temperature rise of 1.940 K. For benzoic acid, the internal energy combustion at constant volume, ∆U, is known to be –3226 kJ/mol. Calculate the calorimeter constant, in kJ/K. b)using the caloremeter constant, determine triangleU, in KJ/mol, for the conbustion of solid biphenyl ((C6H5)2, MW 154.21 g/mol)One mole of a monatomic ideal gas begins in a state withP 5 1.00 atm and T 5 300 K. It is expanded reversiblyand adiabatically until the volume has doubled; then it isexpanded irreversibly and isothermally into a vacuumuntil the volume has doubled again; and then it is heatedreversibly at constant volume to 400 K. Finally, it is compressed reversibly and isothermally until a inal state withP 5 1.00 atm and T 5 400 K is reached. Calculate DSsysfor this process. (Hint: There are two ways to solve thisproblem—an easy way and a hard way.)A sample consisting of 1.00 mol Ar is expanded isothermally at 20 degrees celsius from 10 dm^3 to 30dm^3 (a) reversibly, (b) against a constant external pressure equal to the final pressure of the gas, and (c) freely aka - against zero external pressure. For the three processes calculate q,w, and delta U