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1102-E: Heat Formula 2

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1102-E: Heat Formula 2

BACK to Ladder Heat Transfer and Temperature: Mathematical

$$ Q = m c \Delta T $$

Symbol
Quantity
SI Unit
\( Q \)
Heat Energy Transferred
Joules (J)
\( m \)
mass
kilograms (kg)
\( c \)
Specific Heat of Substance
\( \frac{ \text{J} }{ \text{kg} \cdot ^{\circ} \text{C} } \)
\( \Delta T \)
Change in Temperature
Kelvin (K) or Degrees Celsius (\( ^{\circ} \text{C} \))
Material
Specific heat \( \left( \frac{ \text{J} }{ \text{kg} \cdot ^{\circ} \text{C} } \right) \)
water
4184
oil
1900
wood
1800
aluminum
900
concrete
880
glass
800
steel
470
silver
235
gold
129
  1. When 1500 Joules of energy is lost from a 1.277-kilogram object, its temperature decreases from 45°C to 40°C. What is the specific heat of this object? Of what material is this object made?
  2. What is the specific heat of a material that gains 600 Joules of energy when a 0.25-kilogram object increases in temperature by 3°C? What is this material?
  3. A liquid with a specific heat of 1900 J/kg °C has 4750 Joules of heat energy added to it. Its temperature increases from 20°C to 30°C. What is the mass of the liquid?
  4. What is the mass of a block of concrete that gains 52800 Joules of energy when its temperature is increased by 5°C?
  5. A scientists wants to raise the temperature of a 0.10-kilogram sample of glass from 15°C to 35°C. How much heat energy is required to produce this change in temperature?
  6. A 0.25-kilogram sample of aluminum is provided with 5000 Joules of heat energy. What will be the change in temperature of this sample of aluminum?
  7. What is the change in temperature for a 2-kilogram mass of water than loses 8500 Joules of energy?

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