lead is a soft, dense metal with a specific heat of 0.028 kcal/kg degrees C, a melting point of 328.0 degrees C and a heat of fusion of 5.5 kcal/kg. How much heat must be provided to melt a 250.0 kg sample of lead with a temperature of 20.0 degrees Celsius?
q1 = heat to move the temperature of solid lead from 20.0 degrees C to the melting point of 328.0 degrees C.
q1 = mass x specific heat x delta T.
You have mass, specific heat and temperature difference.
q2=heat to melt the lead at its melting point.
q2 = mass x heat of fusion.
you have mass and you have heat of fusion.
total q = q1 + q2.
Post your work if you get stuck.
3.7235 Kcal
To find the amount of heat required to melt a 250.0 kg sample of lead with a temperature of 20.0 degrees Celsius, we'll need to calculate two separate quantities of heat and then add them together.
First, let's calculate q1, the heat required to raise the temperature of the lead from 20.0 degrees Celsius to its melting point of 328.0 degrees Celsius.
q1 = mass x specific heat x delta T
Let's plug in the given values:
mass = 250.0 kg
specific heat = 0.028 kcal/kg degrees C
delta T = 328.0 degrees C - 20.0 degrees C = 308.0 degrees C
q1 = 250.0 kg x 0.028 kcal/kg degrees C x 308.0 degrees C
Next, let's calculate q2, the heat required to melt the lead at its melting point.
q2 = mass x heat of fusion
Let's plug in the given values:
mass = 250.0 kg
heat of fusion = 5.5 kcal/kg
q2 = 250.0 kg x 5.5 kcal/kg
Finally, let's calculate the total amount of heat required by adding q1 and q2.
total q = q1 + q2
Once you've computed q1 and q2 separately, simply add them together to find the total amount of heat required.
If you need further assistance, please provide the numerical calculations you obtain for q1, q2, and the total q.