The molar heat capacity is given by:
[tex]\begin{gathered} q=nc\Delta T \\ q:heat\text{ }energy \\ n:number\text{ }of\text{ }moles \\ c:molar\text{ }heat\text{ }capacity \\ \Delta T:change\text{ }in\text{ }temperature(T_f-T_i) \end{gathered}[/tex]
We will firstly convert the temperatures to K:
[tex]\begin{gathered} T_f=273.15K+535\degree C=808.15K \\ T_i=273.15K+315\degree C=588.15K \end{gathered}[/tex]
We will substitute the given valuse into the molar heat capacity equation:
[tex]\begin{gathered} q=nc\Delta T \\ q=2.0mol\times25.1J•mol^{-1}•K^{-1}\times(808.15K-588.15K) \\ q=11,044J \\ q=+11.044\text{ }kJ \end{gathered}[/tex]
Answer: The heat absorbed is positive 11.044 kJ,
