Let's break down the problem into simpler steps:

Problem:

You want to find the amount of heat required to raise the temperature of a 1.5 kg object by 120°C. The specific heat capacity of the object is 0.37 calories per gram per degree Celsius (cal/g°C).

Step-by-step solution:

1. Convert mass from kg to grams: Since 1 kg = 1000 grams, the mass of 1.5 kg is: $1.5 \, \text{kg} \times 1000 = 1500 \, \text{grams}$

2. Use the heat formula: The formula to calculate the heat required is: $Q = m \times c \times \Delta T$ where:

   • $Q$ is the heat (in calories),
   • $m$ is the mass (in grams),
   • $c$ is the specific heat capacity (in cal/g°C),
   • $\Delta T$ is the change in temperature (in °C).

3. Plug in the values:

   • $m = 1500 \, \text{g}$,
   • $c = 0.37 \, \text{cal/g°C}$,
   • $\Delta T = 120 \, \text{°C}$.

   So, the heat required is: $Q = 1500 \, \text{g} \times 0.37 \, \text{cal/g°C} \times 120 \, \text{°C}$ $Q = 66600 \, \text{calories}$

Final Answer:

The heat required is 66,600 calories.

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Would you like more details or have any questions?

Here are 5 questions related to this topic:

1. How would the heat change if the mass were 2 kg instead of 1.5 kg?
2. What if the specific heat capacity were 0.50 cal/g°C instead of 0.37 cal/g°C?
3. How does the heat required change if the temperature increase is 100°C instead of 120°C?
4. What is the relationship between mass and heat required when all other factors are constant?
5. Can the specific heat capacity change for the same material under different conditions?

Tip: Always make sure to convert units properly, like kg to grams, when using formulas!