Is the change in enthalpy (ΔH) for dissolution of urea in water positive or negative?

To test the properties of a fertilizer, $$\pu{15.0g}$$ of urea, $$\ce{NH2CONH2_{(s)}}$$, is dissolved in $$\pu{150 mL}$$ of water in a simple calorimeter. A temperature change from $$\pu{20.6^\circ C}$$ to $$\pu{17.8^\circ C}$$ is measured. Calculate the molar enthalpy of solution for the fertilizer urea

I worked through this question by finding $$Q = mc\Delta T$$, and then dividing $$Q$$ by the moles of urea present. I can tell the process is endothermic because $$\Delta T$$ is negative, however my answer for $$\Delta H$$ comes out as negative, which would only make sense if this was an exothermic reaction. I'm not sure where I am wrong to be honest.

Here is my work:

\begin{align} \Delta H &= \frac{(\pu{150ml}) \times (\pu{1g mL^{-1}}) \times (\pu{4.18J g^{-1} K ^{-1}}) \times (\pu{-2.8 K})} {(\pu{15g}/\pu{60.07g})}\\ &= \pu{-7030.59J/mol}\\ &= \pu{-7.03kJ/mol} \end{align}

TL;DR - question asks for $$\Delta H$$ of an endothermic process, not sure if my answer should be positive or negative

In your answer, you are missing a negative sign in $$\Delta H=−Q$$ the way you start out with $$Q$$ from the perspective of the water.