Right now I'm doing a calorimetry lab and for the pre-lab we have been asked to determine the temperature change (in Celsius) of ammonium chloride in water.
The question asks for the expected temperature change ($\Delta T$) of $\pu{8.5 g}$ of $\ce{NH4Cl}$ in $\pu{100 mL}$ (or $\mathrm{g}$) of water, with the molar enthalpy ($\Delta H_\mathrm{sol}$) of the solution being $\pu{0.277 kJ/g}$. The conversion of $\mathrm{kJ/g}$ is throwing me off and I cannot figure out how to solve for $\Delta T$ with the given info.
I know that there are $0.165048...$ moles of solution, which gives me everything I need to solve. We were given the equation
$$n \Delta H_\mathrm{sol} = mC \Delta T,$$
where $m$ - mass of water and $C$ - specific heat capacity of water. I am assuming it needs to be rearranged to
$$\Delta T = \frac{mC}{n\Delta H_\mathrm{sol}}$$
Any help is greatly appreciated and I can explain in further detail if necessary. Sorry for the Celsius, we apparently don't use Kelvin in our calculations.