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Which of the following statement(s) is (or are) true? I. Heat (g) is a state function because AH is a state function and q D ΔΗ II. When 50.0 grams of aluminum at 25.0 °C is placed in 50.0 mL of water at 30.0 °C the water will undergo a smaller temperature change than the aluminum (Csp H20 = 4.184 J/g °C; Csp Aluminum = 0.89 J/g %3D %3D °C) III. When a gas is compressed (AV is negative), the work of the gas is negative since the surroundings is doing work on the system and energy flows out of the system IV. For the reaction 2N2 (g) + 5 - 2N205 (g), the change in --> enthalpy is the same whether the reaction takes place in one step or in a series of steps o II, III and IV OI, II, and IV Il and III

Which of the following statement(s) is (or are) true? I. Heat (g) is a state function because AH is a state function and q D ΔΗ II. When 50.0 grams of aluminum at 25.0 °C is placed in 50.0 mL of water at 30.0 °C the water will undergo a smaller temperature change than the aluminum (Csp H20 = 4.184 J/g °C; Csp Aluminum = 0.89 J/g %3D %3D °C) III. When a gas is compressed (AV is negative), the work of the gas is negative since the surroundings is doing work on the system and energy flows out of the system IV. For the reaction 2N2 (g) + 5 - 2N205 (g), the change in --> enthalpy is the same whether the reaction takes place in one step or in a series of steps o II, III and IV OI, II, and IV Il and III

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Question:** Which of the following statement(s) is (or are) true? I. Heat (q) is a state function because ΔH is a state function and q = ΔH II. When 50.0 grams of aluminum at 25.0 °C is placed in 50.0 mL of water at 30.0 °C, the water will undergo a smaller temperature change than the aluminum (C_sp H₂O = 4.184 J/g°C; C_sp Aluminum = 0.89 J/g°C) III. When a gas is compressed (ΔV is negative), the work of the gas is negative since the surroundings is doing work on the system and energy flows out of the system. IV. For the reaction 2N₂ (g) + 5O₂ --> 2N₂O₅ (g), the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. **Options:** - ○ II, III and IV - ○ I, II, and IV - ○ II and III
Transcribed Image Text:**Question:** Which of the following statement(s) is (or are) true? I. Heat (q) is a state function because ΔH is a state function and q = ΔH II. When 50.0 grams of aluminum at 25.0 °C is placed in 50.0 mL of water at 30.0 °C, the water will undergo a smaller temperature change than the aluminum (C_sp H₂O = 4.184 J/g°C; C_sp Aluminum = 0.89 J/g°C) III. When a gas is compressed (ΔV is negative), the work of the gas is negative since the surroundings is doing work on the system and energy flows out of the system. IV. For the reaction 2N₂ (g) + 5O₂ --> 2N₂O₅ (g), the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. **Options:** - ○ II, III and IV - ○ I, II, and IV - ○ II and III
### Educational Content: Thermodynamics Concepts #### Statements on Thermodynamic Principles **I.** Heat (q) is a state function because ΔH is a state function and q = ΔH. **II.** When 50.0 grams of aluminum at 25.0 °C is placed in 50.0 mL of water at 30.0 °C, the water will undergo a smaller temperature change than the aluminum. - Specific heat capacity of water (C<sub>sp</sub> H<sub>2</sub>O) = 4.184 J/g°C - Specific heat capacity of aluminum (C<sub>sp</sub> Aluminum) = 0.89 J/g°C **III.** When a gas is compressed (ΔV is negative), the work of the gas is negative since the surroundings are doing work on the system and energy flows out of the system. **IV.** For the reaction 2N<sub>2</sub> (g) + 5O<sub>2</sub> → 2N<sub>2</sub>O<sub>5</sub> (g), the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. #### Multiple Choice Option - II, III, and IV - I, II, and IV - II and III - II and IV - All of these are correct --- ### Explanation This content refers to basic principles of thermodynamics, focusing on the concepts of heat as a state function, specific heat capacity, work done by/on gases, and enthalpy changes in chemical reactions. Each statement provides an insight into different aspects of these principles. For understanding, one should be familiar with: - State functions and their significance in thermodynamics. - Specific heat capacity and its implications in heat transfer between substances. - Work done during gas compression or expansion and its relation to energy flow. - Enthalpy and its invariance in path-dependent or path-independent processes.
Transcribed Image Text:### Educational Content: Thermodynamics Concepts #### Statements on Thermodynamic Principles **I.** Heat (q) is a state function because ΔH is a state function and q = ΔH. **II.** When 50.0 grams of aluminum at 25.0 °C is placed in 50.0 mL of water at 30.0 °C, the water will undergo a smaller temperature change than the aluminum. - Specific heat capacity of water (C<sub>sp</sub> H<sub>2</sub>O) = 4.184 J/g°C - Specific heat capacity of aluminum (C<sub>sp</sub> Aluminum) = 0.89 J/g°C **III.** When a gas is compressed (ΔV is negative), the work of the gas is negative since the surroundings are doing work on the system and energy flows out of the system. **IV.** For the reaction 2N<sub>2</sub> (g) + 5O<sub>2</sub> → 2N<sub>2</sub>O<sub>5</sub> (g), the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps. #### Multiple Choice Option - II, III, and IV - I, II, and IV - II and III - II and IV - All of these are correct --- ### Explanation This content refers to basic principles of thermodynamics, focusing on the concepts of heat as a state function, specific heat capacity, work done by/on gases, and enthalpy changes in chemical reactions. Each statement provides an insight into different aspects of these principles. For understanding, one should be familiar with: - State functions and their significance in thermodynamics. - Specific heat capacity and its implications in heat transfer between substances. - Work done during gas compression or expansion and its relation to energy flow. - Enthalpy and its invariance in path-dependent or path-independent processes.
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