In calorimetry the water does the measuring, and $Q = mc\,\Delta T$ is how you read it. Say it: Q equals m c delta-T. $Q$ is the heat that moved, in joules; $m$ is the mass being warmed or cooled, in grams; $c$ is the specific heat capacity in joules per gram per degree Celsius — for liquid water, $4.18\ \mathrm{J/(g\cdot^{\circ}C)}$, the single most quoted number in this course; and $\Delta T$ is the temperature change, in degrees Celsius. The Greek delta is said delta, and it means final minus initial — always in that order, every time it appears.

Two consequences of that order, and the exam lives on both. First, $\Delta T$ is signed: water that cools has a negative $\Delta T$, so $Q$ comes out negative, which is thermochemistry's way of saying the sample handed energy over rather than took it in. Second — and this is the one worth relaxing about — because $\Delta T$ is a DIFFERENCE, a rise of 25 °C is a rise of 25 K exactly. The two scales are offset, not stretched, so the offset subtracts itself away. Grade 12 chemistry quotes $c$ per gram, not per kilogram; a mass handed to you in kilograms is a $\times 1000$ waiting to be missed.