How much heat is needed to raise the temperature of 5.58 kilograms of iron from 20.0°C to 1000.0°C? Specific heat of iron is 450,000 J/(kg x °C). Type the correct answer to 3 significant digits.
heat=mass*specific heat*(Tf-Ti)
558000
To calculate the amount of heat needed to raise the temperature of a substance, you can use the formula:
Q = m * c * ΔT
Where:
Q represents the amount of heat required,
m is the mass of the substance,
c is the specific heat capacity of the substance, and
ΔT is the change in temperature.
In this case, the mass of iron (m) is 5.58 kilograms, the specific heat capacity of iron (c) is 450,000 J/(kg x °C), and the change in temperature (ΔT) is from 20.0°C to 1000.0°C.
Let's substitute these values into the formula and calculate the amount of heat:
Q = 5.58 kg * 450,000 J/(kg x °C) * (1000.0°C - 20.0°C)
First, calculate the difference in temperature:
ΔT = 1000.0°C - 20.0°C = 980.0°C
Now, substitute the values into the formula and solve for Q:
Q = 5.58 kg * 450,000 J/(kg x °C) * 980.0°C
Q ≈ 2,444,400,000 J
Rounded to 3 significant digits, the amount of heat needed to raise the temperature of 5.58 kilograms of iron from 20.0°C to 1000.0°C is approximately 2.44 x 10^9 J.