( Q = (m \times c \times \Delta T) + (M \times C \times \Delta T))

This equation represents the calculation of heat energy absorbed or released during a temperature change in a system consisting of two substances. Let's break it down:

**Q**: Total heat energy absorbed or released.  
**m**: Mass of the first substance.  
**c**: Specific heat capacity of the first substance (energy required to raise 1 kg by 1°C).  
**ΔT**: Change in temperature of the substance (final temperature - initial temperature).  
**M**: Mass of the second substance.  
**C**: Specific heat capacity of the second substance.  
**ΔT**: The change in temperature of the second substance (assumed to be the same as the first substance).

In this scenario, heat energy \(Q\) is the sum of the heat energy absorbed or released by both substances, considering the respective masses and specific heat capacities.

Do you want more details on specific heat calculations or examples?  

Here are 5 related questions to consider:
1. How do you calculate specific heat capacity?
2. How does heat transfer differ between substances with different specific heat capacities?
3. Can this equation be applied to phase changes, like melting or boiling?
4. What happens if the two substances are at different initial temperatures?
5. How does this equation change if there is energy loss to the environment?

**Tip**: The specific heat capacity of water is commonly used in problems (around 4.18 J/g°C), as water often acts as a medium for heat transfer.

Learn how to calculate the total heat energy using the equation Q = (m × c × ΔT) + (M × C × ΔT), where mass, specific heat capacity, and temperature change are key factors. This concept involves thermodynamics and energy transfer, suitable for students in Grades 9-12.

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