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A 2.50 mol sample of an ideal gas for which
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Thermodynamics, Statistical Thermodynamics, & Kinetics
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- For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).arrow_forwardBenzoic 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.arrow_forwardWhat is the change in internal energy when a gas contracts from 377mL to 119mLundera pressure of 1550 torr, whileat the same time being cooled by removing 124.0J ofheat energy?arrow_forward
- The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.arrow_forwardConsider a process in which an ideal gas changes from state 1 to state 2 in such a way that its temperature changes from 300 K to 200 K. (a) Does the temperature change depend on whether the process is reversible or irreversible?arrow_forwardThe molar heat capacities of substances varies with temperature. The general function for determining the molar heat capacity is given below. Cp(a + bT +cT)²R. In case of a gas where a = 3.245, b = 7.108×10^-4 K^-1, and c= -4.06×10^-8 K^-2 for temperatures in the range of 300 Kelvins to 1,500 Kelvins. What is the heat capacity (in joules per kelvin per mole) of this gas at 1,500 Kelvins?arrow_forward
- Five moles of monatomic ideal gas enter the abc cycle and during a complete cycle 600 J of heat is removed from the gas. Process ab is under constant pressure and process bc is increasing at constant volume takes place at pressure. The temperatures of points a and b are Ta= 3°C and Tb= 63°C. What is the work in the ca process?arrow_forward1.65 mol of a perfect gas for which Cv,m = 12.47 J K–1 mol–1 is subjected to two successive changes in state: (1) from 37.0 oC and 1.00´105 Pa, the gas is expended isothermally against a constant pressure of 16.5´103 Pa to twice its initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from 37.0 oC to - 23.0 oC. (a) Calculate q , w , DU, DH for each of the stages.arrow_forwardThe temperature dependence of the molar heat capacity cp of nitrogen can be written as: Ср c₂ = (27.27 +5.22-10³ T/K – 0.0042·10° T²³/K²) J/(K·mol). Calculate the required heat to increase the temperature at constant volume of 1mol N₂ from 273 to 1273 K (mind the difference between c, and c₁).arrow_forward
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