A gas obeying the equation of state p(V − nb) = nRT is subjected to a Joule–Thomson expansion. Will the temperature increase, decrease, or remain the same?
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A gas obeying the equation of state p(V − nb) = nRT is subjected to a Joule–Thomson expansion. Will the temperature increase, decrease, or remain the same?
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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?A) For nitrogen gas the values of Cv and Cp at 25°C are 20.8 J K−1 mol−1 and 29.1 J K−1 mol−1, respectively. When a sample of nitrogen is heated at constant pressure, what fraction of the energy is used to increase the internal energy of the gas? B) How much energy (in KJ) is required to raise the temperature of 136.4 g N2 from 25.0°C to 87.0°C in a vessel having a constant volume?Estimate the enthalpy of vaporization of water at 100 °c from its value at 25 °c, 44.01 kJ mol-1, given the constant pressure molar heat capacities of 75.29 J K-1 mol-1 and 33.58 J K-1 mol-1 for liquid and gas, respectively.
- Nitrogen gas stored in a flexible container expanded from a volume of 500 dm3 to a volume of 600 dm3 at a constant external pressure of 101.3 kPa upon absorbing 35.5 kJ of heat. How much is the change in the internal energy of the gas?When 229 J of energy is supplied as heat to 3.00 mol Ar(g), the temperature of the sample increases by 2.55 K. Calculate the molar heat capacities at constant volume and constant pressure of the gas.For CO_2 how would the theoretical ratio of C_p (heat capacity at constant pressure)/ C_v (heat capacity at constant volume) be affected if the molecule were nonlinear, such as SO_2, instead of linear? Could you decide between these two structures from the C_p/C_v ratio alone?
- molar enthalpy of formation of H2O(l) from its elements in their standard states (25 oC and 100 kPa)?What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 KK? Express your answer to three significant figures and include the appropriate units.1. In an isobaric system, one (1) mole of monoatomic ideal gas at 25 °C was heated, then undergoes expansion against a constant external pressure of 1 atm until the initial volume of 1 L become 10 L. Calculate: a) Temperature T2 b) Work, w c) Internal Energy, AU d) Enthalpy, AH. e) Heat , q
- When 229 J of energy is supplied as heat at constant pressure to 3.0 mol Ar(g) the temperature of the sample increases by 2.55 K. Calculate the molar heat capacities at constant volume and constant pressure of the gas.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?For the combustion of 1.00 mol of benzene, C6H6 (∆Hf° = 49.1 kJ/mol), at 25 °C and 1.00 bar Calculate the work that must be done against the atmosphere for the expansion of the gaseous products.