How much heat is required to melt 0.163 kg of lead at 327.3°C?
To calculate the heat required to melt a given amount of lead, we can use the formula: Q = m * L. Where:
- Q is the heat required (in joules)
- m is the mass of the lead (in kilograms)
- L is the specific heat of fusion for lead (in joules per kilogram, J/kg)
Given:
- Mass of lead, m = 0.163 kg
- Specific heat of fusion for lead, L = 24.5 × 10^3 J/kg
Substituting the given values into the formula:
Q = 0.163 kg * 24.5 × 10^3 J/kg
Q = 3.9995 × 10^3 J
Therefore, approximately 3.9995 × 10^3 joules (or 3999.5 joules) of heat are required to melt 0.163 kg of lead at 327.3°C.
Explaining the Calculation
Formula:
The formula Q = m * L is used to calculate the heat required to melt a substance. In this case, we are calculating the heat required to melt lead.
Given Values:
Mass of lead (m): 0.163 kg
Specific heat of fusion for lead (L): 24.5 × 10^3 J/kg
Calculation:
By substituting the given values into the formula, we get:
Q = 0.163 kg * 24.5 × 10^3 J/kg
Q = 3.9995 × 10^3 J
Therefore, approximately 3.9995 × 10^3 joules (or 3999.5 joules) of heat are required to melt 0.163 kg of lead at 327.3°C.
Conclusion:
Calculating the heat required to melt lead involves using the mass of the lead and the specific heat of fusion for lead. By plugging in the values into the formula, we can determine the amount of heat needed for the process.