how much energy i kj is required to change the temp of 1.00 kg of fe from 25.0 degrees celsius to 1515 degrees celsius?
mass*sph*dt
so it would be q= (.449)(1.00)(1490)?
no
To calculate the amount of energy required to change the temperature of a substance, you can use the equation:
Q = m * c * ΔT
Where:
Q is the energy transferred (in joules),
m is the mass of the substance (in kg),
c is the specific heat capacity of the substance (in J/kg°C), and
ΔT is the change in temperature (in °C).
In this case, you have a mass of 1.00 kg of iron (Fe), and you want to calculate the energy required to heat it from 25.0 degrees Celsius to 1515 degrees Celsius.
First, you need to know the specific heat capacity of iron. The specific heat capacity of iron is approximately 450 J/kg°C.
Next, calculate the change in temperature:
ΔT = final temperature - initial temperature
= 1515°C - 25.0°C
= 1490°C (or 1490 K)
Now plug in the values into the equation:
Q = m * c * ΔT
= 1.00 kg * 450 J/kg°C * 1490 K
Calculating the result:
Q ≈ 670,500 J
To convert this value to kilojoules (kJ), divide by 1000:
Q ≈ 670.5 kJ
Therefore, approximately 670.5 kJ of energy is required to change the temperature of 1.00 kg of iron from 25.0°C to 1515°C.