The contributions to the molar heat capacity of a N2(g) at 273 K are: (A) Cv(translational) < Cv(rotational) < Cv(vibrational) (B) Cv(vibrational) < Cv(rotational) < Cv(translational) (C) Cv(rotational) < Cv(vibrational) < Cp(translational) (D) Cv(rotational) < Cv (translational) < Cv(vibrational)
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- Calculate the vibrational, rotational, and translational contributions to the constant volume heat capacity (Cv) for 14N2 at 298 K. Assume this represents the high temperature limit for rotational energy and low temperature limit for vibrational energy. Given that Cv=20.81 J/K·mol for N2, state which type or types of energy contribute most to Cv for N2 and explain why those types of energy contribute most.1.3 The ground level of Cl is 2P3/2 and a 2P1/2 level lies 881 cm-1 there above. Calculate the electronic contribution to the heat capacity of Cl atoms at 500 K.Use the equipartition principle to estimate the values of γ = Cp/CV for gaseous ammonia and methane. Do this calculation with and without the vibrational contribution to the energy. Which is closer to the experimental value at 25 °C?
- How much energy does it take to raise the temperature of 1.0 mol H2O(g) from 100 °C to 200 °C at constant volume? Consider only translational and rotational contributions to the heat capacity.Use the equipartition theorem to estimate the constant-volume molar heat capacity of (i) I2, (ii) CH4, (iii) C6H6 in the gas phase at 25 °C.Find the potential energy for two methyl chloride molecules at 25°C seperated by 1.9°C
- A linear molecule may rotate about two axes. If the molecule consists of N atoms, then there are 3N- 5 vibrational modes. Use the equipartition theorem to estimate the total contribution to the molar internal energy from translation, vibration, and rotation for (a) carbon dioxide, CO2, and (b) dibromoethyne, C2Br2, at 2000 K. In contrast, a nonlinear molecule may rotate about three axes and has 3N- 6 vibrational modes. Estimate the total contribution to the molar in ternal energy from translation, vibration, and rotation for (c) nitrogen dioxide, NO2, and (d) tetrabromoethene, C2Br4,at 2000 K. In each case, first assume that all vibrations are active; then assume that none is.Use the equipartition theorem to estimate the constant- volume molar heat capacity of (i) O3, (ii) C2H6, (iii) CO2 in the gas phase at 25 °C.Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen. Given the following reaction and associated data at T = 298.15 K. 2 H(g) ⇌ H"(g) or equivalently H(g) + H(g) ⇌ H2(g) Δf?° (kJ mol-1) ?° (kJ K-1 mol-1) H(g) 218.0 0.115 H2(g) 0 0.131 Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K. Calculate KP for the reaction. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.
- 1. Use the equipartition principle to estimate the value of γ = Cpm/CVm for gaseous N2O5. Do this calculation WITH the vibrational contribution to the energy. 2. A sample consisting of 0.15 mol of gas is compressed isothermally at 300K from 0.02m3 to 0.01m3 reversibly. Calculate w. 3. A sample consisting of 3 mol of argon (monoatomic gas), initially at P1=352kPa and T1= 320K, is cooled reversibly to 240K at constant volume. Calculate the q. 4. A chemical reaction takes place in a container fitted with a piston of cross-sectional area 20cm2. As a result of the reaction, the gas undergoes a compression, the piston is displaced by 5cm (toward the bottom of the container), pushed by an external pressure of 105Pa. Calculate the work.N2O and CO2 have similar rotational constants (12.6 and 11.7 GHz, respect ively) but strikingly different rotational partition functions. Why?Calculate the contribution of each normal mode to the molar vibrational heat capacity of H_2O (g) at 600 K.