How many calories of heat are needed to increase the temperature of 55 g of ethanol from 18 Celsius to 48 Celsius
961.95 cal
To calculate the calories of heat needed to increase the temperature of a substance, we can use the formula:
Q = m * C * ΔT
Where:
Q is the heat energy in calories,
m is the mass of the substance in grams,
C is the specific heat capacity of the substance in calories per gram per degree Celsius, and
ΔT is the change in temperature in degrees Celsius.
First, we need to determine the specific heat capacity of ethanol. The specific heat capacity of ethanol is approximately 2.44 calories per gram per degree Celsius.
Calculating the heat energy:
Q = 55 g * 2.44 cal/g°C * (48°C - 18°C)
Q = 55 * 2.44 * 30
Q ≈ 4,026 calories
Therefore, approximately 4,026 calories of heat energy are needed to increase the temperature of 55 g of ethanol from 18°C to 48°C.