Heat Transfer and Thermal Equilibrium Practice Test

A 30.0 g piece of metal at $10^\circ\text{C}$ is placed into 120.0 g of water at $40^\circ\text{C}$ in an insulated container. The specific heats are $c_{\text{metal}}=0.80\ \text{J g}^{-1}!!\cdot!^\circ\text{C}^{-1}$ and $c_{\text{water}}=4.18\ \text{J g}^{-1}!!\cdot!^\circ\text{C}^{-1}$. Heat lost equals heat gained. Which statement is correct about the signs of $q$ for each substance (taking $q>0$ as heat gained by the substance)?

A $50.0,\text{g}$ piece of metal at $120^\circ\text{C}$ (specific heat capacity $c=0.50,\text{J},\text{g}^{-1},\text{^\circC}^{-1}$) is placed into $100.0,\text{g}$ of water at $20.0^\circ\text{C}$ ($c=4.18,\text{J},\text{g}^{-1},\text{^\circC}^{-1}$) in an insulated container. Assume no heat is lost to the surroundings, so heat lost by the metal equals heat gained by the water. Which statement best describes the direction of heat flow and the final equilibrium temperature?