Thermodynamics and Enthalpy - Higher Difficulty Problems
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Q. Calculate the enthalpy change (ΔH) for the reaction: 2NO(g) + O2(g) → 2NO2(g) given the following bond enthalpies: N≡N = 941 kJ/mol, O=O = 498 kJ/mol, N=O = 201 kJ/mol.
Q. For a reaction at equilibrium, if the temperature is increased and ΔH is positive, what will happen to the position of equilibrium?
Q. For the reaction A + B ⇌ C + D, if ΔH = -150 kJ and ΔS = -200 J/K, what is the temperature at which the reaction becomes non-spontaneous?
Q. In a calorimetry experiment, if 50 g of water is heated from 25 °C to 75 °C, what is the heat absorbed (q) assuming specific heat capacity of water is 4.18 J/g°C?
Q. In a closed system, if 100 J of heat is added to a gas and it does 40 J of work, what is the change in internal energy (ΔU) according to the first law of thermodynamics?
Q. In an isothermal process for an ideal gas, if the volume of the gas is doubled, what happens to the pressure?
Q. What is the change in enthalpy (ΔH) for the reaction: 2H2(g) + O2(g) → 2H2O(g) if the bond enthalpies are: H-H = 436 kJ/mol, O=O = 498 kJ/mol, H-O = 463 kJ/mol?
Q. What is the Gibbs free energy change (ΔG) at 298 K for a reaction with ΔH = -100 kJ and ΔS = -200 J/K?
Q. What is the standard enthalpy change (ΔH°) for the formation of 1 mole of CO2(g) from C(s) and O2(g) given the following reactions: C(s) + O2(g) → CO2(g) ΔH° = -393.5 kJ?
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