Which of the following statements is/are true?
(I) q (heat) is a state function because ΔH is a state function and q=Δ .
(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. (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 is doing work on the system and energy flows out of the system.
(IV) For the reaction (at constant pressure) 2N₂(g) +5O₂(g) → 2N₂O₅(g) , the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps.

Question

Quizplus · Accepted Answer

- Statement I is false because q (heat) is not a state function; it depends on the path taken, whereas ΔH (enthalpy change) is a state function.- Statement II is true because water (H2O) has a higher specific heat capacity than aluminum, meaning it requires more energy to change its temperature, so aluminum will undergo a larger temperature change.- Statement III is false because when a gas is compressed and work is done on the system, the work is positive (according to the convention that work done on the system is positive), and energy flows into the system, not out.- 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 taken to get from reactants to products.

Which of the Following Statements Is/are True