Question

Calculate the amount of heat, in calories, that must be added to warm 89.7 g

of ethanol (0.58) from 22.0 °C
to 44.1 °C.
Assume no changes in state occur during this change in temperature.

Answer 1

The specific heat capacity of ethanol is 2.44 J/(g°C). Converting this to calories/(g°C), we get:

2.44 J/(g°C) x (1 cal/4.184 J) = 0.582 cal/(g°C)

Using this specific heat capacity, we can calculate the amount of heat required to raise the temperature of 89.7 g of ethanol from 22.0°C to 44.1°C:

Q = m x c x ΔT

where Q is the amount of heat in calories, m is the mass in grams, c is the specific heat capacity in cal/(g°C), and ΔT is the change in temperature in °C.

Plugging in the values, we get:

Q = (89.7 g) x (0.582 cal/(g°C)) x (44.1°C - 22.0°C)
Q = 231.6 cal

Therefore, the amount of heat that must be added to warm 89.7 g of ethanol from 22.0°C to 44.1°C is 231.6 calories.