Which of the following statements is/are true? I.q (heat) is a state function because $\Delta$ H is a state function and q = $\Delta$ H.
II.When 50.0 g of aluminum at 20.0°C is placed in 50.0 mL of water at 30.0°C,the H₂O will undergo a smaller temperature change than the aluminum.(The density of H₂O = 1.0 g/mL,specific heat capacity of H₂O = 4.18 J/g°C,specific heat capacity of aluminum = 0.89 J/g°C)
III.When a gas is compressed,the work is negative since the surroundings are doing work on the system and energy flows out of the system.
IV.For the reaction (at constant pressure) 2N₂(g) + 5O₂(g) $\to$ 2N₂O₅(g) ,the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps.

Question

Which of the following statements is/are true? I.q (heat) is a state function because

\Delta

H is a state function and q =

\Delta

H.
II.When 50.0 g of aluminum at 20.0°C is placed in 50.0 mL of water at 30.0°C,the H₂O will undergo a smaller temperature change than the aluminum.(The density of H₂O = 1.0 g/mL,specific heat capacity of H₂O = 4.18 J/g°C,specific heat capacity of aluminum = 0.89 J/g°C)
III.When a gas is compressed,the work is negative since the surroundings are doing work on the system and energy flows out of the system.
IV.For the reaction (at constant pressure) 2N₂(g) + 5O₂(g)

\to

2N₂O₅(g) ,the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps.

Quizplus · Accepted Answer

- Statement I is incorrect because heat (q) is not a state function; it depends on the path taken to reach a state, not just the initial and final states. Enthalpy ($\Delta H$) is a state function, not heat.- Statement II is true because water, with a higher specific heat capacity, will undergo a smaller temperature change compared to aluminum when the same amount of heat is transferred.- Statement III is incorrect because when a gas is compressed and work is done on the system, energy flows into the system, not out. The work is considered negative from the system's perspective according to the convention that work done by the system is positive.- Statement IV is true due to Hess's Law, which states that the total enthalpy change for a reaction is the same, regardless of the number of steps it takes to get from reactants to products.

Which of the Following Statements Is/are True? I Δ\DeltaΔ H Is a State Function and Q =

Which of the Following Statements Is/are True? I $\Delta$ H Is a State Function and Q =