What is the heat required to raise the temperature of a 1.5 kg mass by 120°C if the specific heat of the mass is 0.37 cal./g. °C?

To find the heat required, we can use the formula:

\[
Q = mc\Delta T
\]

where:
- \( Q \) is the heat energy required,
- \( m \) is the mass of the object,
- \( c \) is the specific heat capacity of the material,
- \( \Delta T \) is the change in temperature.

Let's plug in the given values:
- \( m = 1.5 \, \text{kg} = 1500 \, \text{g} \) (since 1 kg = 1000 g),
- \( c = 0.37 \, \text{cal/g°C} \),
- \( \Delta T = 120 \, \text{°C} \).

Now calculate the heat \( Q \):

\[
Q = (1500 \, \text{g}) \times (0.37 \, \text{cal/g°C}) \times (120 \, \text{°C})
\]

\[
Q = 1500 \times 0.37 \times 120
\]

\[
Q = 66,600 \, \text{cal}
\]

So, the heat required to raise the temperature is **66,600 calories**.

Would you like more details or have any questions about this calculation?

Here are five related questions you might find interesting:
1. How would the heat required change if the mass were doubled?
2. What happens to the heat required if the specific heat capacity changes to 0.50 cal/g°C?
3. How much heat is required if the temperature change is only 60°C?
4. What is the specific heat in joules if 1 cal = 4.184 J?
5. How would the heat calculation differ if the mass was given in pounds instead of kilograms?

**Tip**: Always make sure to convert units consistently when performing calculations in different systems (e.g., grams vs kilograms).

Find out how to calculate the heat required to raise the temperature of a 1.5 kg mass by 120°C, using the specific heat formula Q = mcΔT. This problem involves thermodynamics and heat transfer concepts, with a step-by-step solution. Suitable for students in Grades 9-12.

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