Which of the following constants is/are needed to calculate the amount of energy required to heat 30.5g of H₂O(s) at -25.0^$\circ$C to H₂O(l) at 55.0^$\circ$C
I. $\Delta$ H_fus (H₂O)
II. $\Delta$ H_vap (H₂O)
III. specific heat of H₂O(s)
IV. specific heat of H₂O(l)
V. specific heat of H₂O(g)

Question

Which of the following constants is/are needed to calculate the amount of energy required to heat 30.5g of H₂O(s) at -25.0^$\circ$C to H₂O(l) at 55.0^$\circ$C
I.

\Delta

H_fus (H₂O)
II.

\Delta

H_vap (H₂O)
III. specific heat of H₂O(s)
IV. specific heat of H₂O(l)
V. specific heat of H₂O(g)

Quizplus · Accepted Answer

I, III, and IVTo calculate the energy required to heat a substance from a solid at a sub-zero temperature to a liquid at a higher temperature, you need the heat of fusion (I) to convert the solid to liquid, the specific heat of the solid (III) to heat it up to its melting point, and the specific heat of the liquid (IV) to heat the liquid to the desired temperature. The heat of vaporization (II) and the specific heat of the gas phase (V) are not needed since the substance does not enter the gas phase in this scenario.

Which of the Following Constants Is/are Needed to Calculate the Amount