In a constant-volume calorimeter, 17.5 moles of an ideal gas cools from 75.3oC to 25.0oC. Calculate w, q, ∆U, and ∆H for the process [CV
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One mole of an ideal gas with Cv=3/2R is subjected to two successive changes in state: (1) From 25.0°C and 100 x 10^3 Pa, the gas is expanded isothermally against a constant pressure of 20.0 x 10^3 Pa to twice the initial volume; (2) the gas is cooled at constant volume from 25.0°C to -25.0°C. Calculate q, w, delta U, and delta H for each of the stages and also for the complete process.
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A 2.50 mole sample of an ideal gas, for which $C_{V, m}=3 R / 2,$ is subjected to two successive changes in state: (1) From $25.0^{\circ} \mathrm{C}$ and $125 \times 10^{3} \mathrm{Pa}$, the gas is expanded isothermally against a constant pressure of $15.2 \times 10^{3} \mathrm{Pa}$ to twice the initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from $25.0^{\circ} \mathrm{C}$ to $-29.0^{\circ} \mathrm{C} .$ Calculate $q, w, \Delta U,$ and $\Delta H$ for each of the stages. Also calculate $q, w, \Delta U,$ and $\Delta H$ for the complete process.
1.65 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 °C and 1.00×105 Pa, the gas is expanded 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 °C to -23.0 °C. (a) Calculate q, w, ΔU, ΔH for each of the stages.
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