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Calculate the contribution that rotational motion makes to the molar entropy of a gas of HCl molecules at 25 °C.
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- Determine an expression for V/T p, n in terms of and . Does the sign on the expression make sense in terms of what you know happens to volume as temperature changes?At what temperature is the standard molar entropy of helium equal to that of xenon at 298 K?Calculate the molar entropy of a constant-volume sample of argon at 270 K given that it is 154.84 J K–1 mol–1 at 298 K. Unit in J/mol-K.
- At what temperature is the translational contribution to the standard molar entropy of CO2(g) equal to that of H2O(g) at 298 K?Estimate the increase in the molar entropy of O2(g) when the temperature is increased at constant pressure from 298 K to 348 K, given that the molar constant-pressure heat capacity of O2 is 29.355 J K−1 mol−1 at 298 K.Calculate the translational contribution to the standard molar entropy at 298 K of (i) H2O(g), (ii) CO2(g).
- Calculate the molar entropy of a constant-volume sample of argon at 250 K given that it is 154.84 J K−1 mol−1 at 298 K; the molar constant-volume heat capacity of argon is 3/2 R.The molar entropy of a sample of neon at 298 K is 146.22 J K−1 mol−1. The sample is heated at constant volume to 500 K; assuming that the molar constant-volume heat capacity of neon is 3/2 R, calculate the molar entropy of the sample at 500 K.Suppose that the weight, W, of a configuration of N molecules in a gas of volume V is proportional to VN. Use Boltzmann's formula to deduce the change in entropy when the gas expands isothermally from Vi to Vf.
- What is the basis for deriving an expression for entropy as a function of temperature and volume? Internal energy Enthalpy Gibbs energy Helmholtz energyCalculate the change in the entropies of the system and the surroundings, and the total change in entropy, when the volume of a sample of argon gas of mass 31.5 g at 298 K and 1.50 bar increases from 1.20 L to 4.60 L in an adiabatic reversible expansion.Derive an expression for the heat capacity at constant pressure Cp in terms of thermodynamic variables (N,V,P,T) by differentiating the enthalpy with respect to the temperature. How does Cp vary during free expansion of the ideal gas?