How much energy would be required to heat 60 grams of water from -50 degrees C to 200 degrees C?
To calculate the amount of energy required to heat a substance, you can use the specific heat capacity formula:
Energy = mass × specific heat capacity × temperature change
In this case, the substance is water, and its specific heat capacity is approximately 4.18 J/g°C. Keep in mind that the units for mass and specific heat capacity should be consistent (both in grams or both in kilograms).
Step 1: Convert the temperature from degrees Celsius (°C) to Kelvin (K).
To convert from degrees Celsius to Kelvin, add 273.15 to the temperature in °C.
Initial temperature (T1) = -50°C + 273.15 = 223.15 K
Final temperature (T2) = 200°C + 273.15 = 473.15 K
Step 2: Calculate the temperature change (∆T).
∆T = T2 - T1 = 473.15 K - 223.15 K = 250 K
Step 3: Plug in the values into the specific heat capacity formula.
Energy = mass × specific heat capacity × temperature change
Given:
mass of water = 60 grams
specific heat capacity of water = 4.18 J/g°C
temperature change (∆T) = 250 K
Energy = 60 g × 4.18 J/g°C × 250 K
Step 4: Calculate the energy required.
Energy = 627,000 J or 627 kJ (rounded to the nearest kilojoule)
Therefore, it would require approximately 627 kilojoules of energy to heat 60 grams of water from -50°C to 200°C.