(a) How much heat is required to raise by 12.40°C the temperature of 1.4 kg of water.
(b) How much heat is required to raise by 12.40°C the temperature of 1.4 kg of iron.
Q =c•m•Δt,
where c is the heat capacity for
Water (liquid): c = 4185.5 J/(kg•K), and for Iron: c = 4500 J/(kg•K)
To find the amount of heat required to raise the temperature of a substance, we can use the formula:
Q = m * C * ΔT
Where:
Q is the amount of heat in Joules (J)
m is the mass of the substance in kilograms (kg)
C is the specific heat capacity of the substance in Joules per kilogram per degree Celsius (J/kg°C)
ΔT is the change in temperature in degrees Celsius (°C)
(a) Heat required to raise the temperature of 1.4 kg of water by 12.40°C:
First, we need to find the specific heat capacity of water. The specific heat capacity of water is approximately 4186 J/kg°C.
Substituting the values into the formula:
Q = m * C * ΔT
Q = 1.4 kg * 4186 J/kg°C * 12.40°C
Q ≈ 70,565.92 J
So, approximately 70,565.92 Joules (J) of heat is required to raise the temperature of 1.4 kg of water by 12.40°C.
(b) Heat required to raise the temperature of 1.4 kg of iron by 12.40°C:
The specific heat capacity of iron is approximately 450 J/kg°C.
Substituting the values into the formula:
Q = m * C * ΔT
Q = 1.4 kg * 450 J/kg°C * 12.40°C
Q ≈ 8,316 J
So, approximately 8,316 Joules (J) of heat is required to raise the temperature of 1.4 kg of iron by 12.40°C.