When two bodies at different temperatures $T_1$ and $T_2$ are brought in thermal contact, they attain thermal equilibrium at a common temperature. However, this final temperature is not necessarily the mean $(T_1 + T_2)/2$ because the two bodies may have different heat capacities. As noted in the context, $\Delta Q$ is proportional to the total mass of the system and is extensive. The body with larger heat capacity will undergo a smaller temperature change for the same heat transfer. The final equilibrium temperature depends on the ratio of heat capacities, not simply on the temperatures.

A coolant with high specific heat can absorb a large amount of heat for a given temperature rise. From the context, $\Delta Q$ is clearly proportional to the total mass of system and hence is extensive. A coolant having high specific heat capacity can absorb more heat energy ($\Delta Q$) without significant temperature increase, making it more effective in preventing different parts of the plant from getting too hot.

During driving, the air inside the tyre gets heated due to friction and other dissipative effects. The context mentions that dissipative effects are present everywhere and lead to loss of mechanical energy as heat. The context also refers to the ideal gas relation as the equation of state. For an ideal gas at constant volume, pressure is directly proportional to temperature. As temperature increases, the pressure inside the tyre increases accordingly.

The context mentions that $\Delta Q$ is proportional to the total mass and is extensive. Water has high specific heat capacity compared to land. A harbour town is surrounded by water which can absorb large amounts of heat without significant temperature change. This moderates the climate. In contrast, a desert town has land (sand) with low specific heat, causing large temperature variations between day and night, making the climate less temperate.