How much (in Celsius degrees) is the temperature of 1.3 kg of alcohol raised by adding 4.1 kcal of heat? The following piece of information may come in handy: specific heat of alcohol is 0.58 kcal/kgC.
To find the change in temperature of the alcohol, we can use the formula:
Q = m * c * ΔT
Where:
Q is the heat energy transferred
m is the mass of the substance
c is the specific heat capacity
ΔT is the change in temperature
In this case, we know:
Q (heat energy transferred) = 4.1 kcal
m (mass of alcohol) = 1.3 kg
c (specific heat capacity of alcohol) = 0.58 kcal/kg°C
ΔT (change in temperature) is what we need to find.
Rearranging the formula, we get:
ΔT = Q / (m * c)
Plugging in the values, we have:
ΔT = 4.1 kcal / (1.3 kg * 0.58 kcal/kg°C)
To calculate this, divide 4.1 by the product of 1.3 and 0.58:
ΔT = 4.1 / (1.3 * 0.58)
Simplifying further:
ΔT = 4.1 / 0.754
Using division, we find:
ΔT ≈ 5.43 °C
Therefore, the temperature of 1.3 kg of alcohol would be raised by approximately 5.43 degrees Celsius by adding 4.1 kcal of heat.