the specific heat of ice is 0.5 cal/g degrees c. which will require more heat: heating 100g of ice to 20 degrees c, or heating 100g of liquid water to 20 degrees c?
To determine which will require more heat, we need to calculate the amount of heat required for each scenario.
1. Heating 100g of ice to 20 degrees Celsius:
To calculate the heat required, we can use the formula:
Q = m * C * ΔT
Where:
Q is the heat energy
m is the mass
C is the specific heat
ΔT is the change in temperature
For ice:
m = 100g
C = 0.5 cal/g°C
ΔT = (20 - 0) = 20°C
Q = (100g) * (0.5 cal/g°C) * (20°C) = 1000 cal
2. Heating 100g of liquid water to 20 degrees Celsius:
Similarly, we can use the same formula:
For liquid water:
m = 100g
C = 1 cal/g°C (specific heat of water)
ΔT = (20 - 0) = 20°C
Q = (100g) * (1 cal/g°C) * (20°C) = 2000 cal
From the calculations, it is evident that heating 100g of liquid water to 20 degrees Celsius requires more heat compared to heating 100g of ice to the same temperature.
To determine which requires more heat, we need to calculate the amount of heat energy required for each scenario. The equation used is:
Q = m * c * ΔT
Where:
Q = heat energy (in calories)
m = mass (in grams)
c = specific heat capacity (in cal/g°C)
ΔT = change in temperature (in °C)
Let's calculate the heat energy required for each scenario:
For heating 100g of ice to 20°C:
Q_ice = 100g * 0.5 cal/g°C * (20°C - 0°C)
Q_ice = 100g * 0.5 cal/g°C * 20°C
Q_ice = 1000 cal
For heating 100g of liquid water to 20°C:
Q_water = 100g * 1 cal/g°C * (20°C - 0°C)
Q_water = 100g * 1 cal/g°C * 20°C
Q_water = 2000 cal
Therefore, heating 100g of liquid water to 20°C requires more heat (2000 cal) compared to heating 100g of ice to 20°C (1000 cal).