Textbook Problem

If the heat capacity varies with temperature, a better form of equation 2.9 is to solve

$\mathrm{q}=\underset{{\mathrm{T}}_{\mathrm{i}}}{\overset{{\mathrm{T}}_{\mathrm{f}}}{\int }}\mathrm{n}\stackrel{-}{\mathrm{C}\left(\mathrm{T}\right)}d\mathrm{t}$

A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is $\stackrel{-}{\mathrm{C}\left(\mathrm{T}\right)}$ = 56.99+0.1202T J/mol.K, how much heat is needed?