a student reverses the thermochemical equation below. s(s) + o₂(g) → so₂(g) δh = -297 kj what is the correct…

a student reverses the thermochemical equation below. s(s) + o₂(g) → so₂(g) δh = -297 kj what is the correct change in enthalpy for the reversed equation? drag these tiles and drop them in the correct blank above -297 kj 297 kj 594 kj -594 kj

a student reverses the thermochemical equation below. s(s) + o₂(g) → so₂(g) δh = -297 kj what is the correct change in enthalpy for the reversed equation? drag these tiles and drop them in the correct blank above -297 kj 297 kj 594 kj -594 kj

Answer

Explanation:

Step1: Recall thermochemistry rule

When a thermochemical equation is reversed, the sign of $\Delta H$ changes.

Step2: Apply rule to given $\Delta H$

The original $\Delta H=- 297$ kJ. For the reversed equation, $\Delta H = 297$ kJ.

Answer:

297 kJ