104 Created by Kamran FatehThermodynamics and Thermochemistry Quiz Batch 07Thermodynamics studies energy, heat, and work, focusing on their transformations in physical and chemical processes. Thermochemistry deals with heat changes in chemical reactions, determining whether they are exothermic or endothermic. 1 / 27The specific heat of water is: a) 2.05 J/g°C b) 4.18 J/g°C c) 0.90 J/g°C d) 1.00 J/g°C 2 / 27If ΔG∘=−RTlnK, and K=1, then ΔG∘ is: Zero Positive Negative Undefined 3 / 27Hess’s Law states that: a) Enthalpy is a state function b) The enthalpy change of a reaction is the sum of the enthalpy changes of individual steps c) Entropy always increases d) Gibbs free energy determines spontaneity 4 / 27Entropy (S) is a measure of: a) Heat content b) Disorder c) Enthalpy d) Work done 5 / 27For a reaction with ΔH<0 and ΔS>0, the reaction is: a) Spontaneous at all temperatures b) Spontaneous only at high temperatures c) Spontaneous only at low temperatures d) Nonspontaneous at all temperatures 6 / 27What does thermodynamics study? a) Speed of reactions b) Interrelation of heat, work, energy, and entropy c) Molecular structures d) Atomic masses 7 / 27In a bomb calorimeter, the heat transfer is measured under: a) Constant volume b) Constant pressure c) Variable temperature d) Variable pressure 8 / 27Enthalpy (H) is defined as: a) The heat content of a substance b) The work done by a system c) The entropy of a system d) The internal energy of a system 9 / 27The bond enthalpy is the energy required to: a) Break a bond b) Form a bond c) Measure entropy d) Calculate Gibbs free energy 10 / 27Hess’s Law is used to: a) Calculate Δ H for a reaction using multiple steps b) Measure entropy c) Determine Gibbs free energy d) Calculate heat capacity 11 / 27The phase change from solid to gas is called: a) Sublimation b) Deposition c) Vaporization d) Fusion 12 / 27The heat of fusion is the energy required for: a) Solid to liquid b) Liquid to gas c) Gas to solid d) Liquid to solid 13 / 27The Gibbs free energy equation is: a) Δ G = Δ H + T Δ S b) Δ G = Δ H − T Δ S c) Δ G = Δ S − T Δ H d) Δ G = Δ H / T Δ S 14 / 27The equation ΔE=q+w represents: a) The second law of thermodynamics b) The first law of thermodynamics c) Gibbs free energy d) Entropy change 15 / 27The first law of thermodynamics states: a) Entropy always increases b) Energy cannot be created or destroyed c) Absolute zero cannot be achieved d) Gibbs free energy determines spontaneity 16 / 27For a reaction with ΔS>0: a) The system becomes more ordered b) The system becomes more disordered c) The enthalpy decreases d) The Gibbs free energy increases 17 / 27Which state of matter has the highest entropy? a) Solid b) Liquid c) Gas d) Plasma 18 / 27The second law of thermodynamics states a) Energy is conserved b) Entropy of the universe always increases c) Enthalpy is a state function d) Work is path-dependent 19 / 27Which of the following is NOT part of the surroundings? a) The reaction flask b) The air outside the flask c) The reactants d) The table holding the flask 20 / 27Which term is NOT a state function? a) Enthalpy (H) b) Entropy (S) c) Heat (q) d) Internal energy (E) 21 / 27The phase change from gas to solid is called: a) Sublimation b) Deposition c) Condensation d) Freezing 22 / 27Which phase change is endothermic? a) Freezing b) Condensation c) Melting d) Deposition 23 / 27State functions depend on: a) The pathway of the process b) Initial and final states only c) Temperature and pressure d) Volume changes 24 / 27A reaction is spontaneous if: a) Δ G > 0 b) Δ G < 0 c) Δ G = 0 d) Δ H = 0 25 / 27The third law of thermodynamics states: a) Entropy of a perfect crystal at 0 K is zero b) Energy is conserved c) Enthalpy is path-independent d) Gibbs free energy must be negative 26 / 27The units of entropy are: a) J/K b) kJ/mol c) J/g°C d) cal/°C 27 / 27If K>1, then ΔG∘ is: a) Positive b) Negative c) Zero d) Cannot be determined Your score isThe average score is 66% 0% Restart quiz
