How much energy, in joules, is needed to heat 100.0 g of ethyl alcohol from 22.0°C to 60°C? The specific heat of ethyl alcohol is 2.44 J/g°C.

The energy is 9,272 J (Joules)

Explanation:

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

In this way, there is a direct proportional relationship between heat and temperature (Two magnitudes are directly proportional when there is a constant so that when one of the magnitudes increases, the other also; and the same occurs when one of the two decreases .). The constant of proportionality depends on the substance that constitutes the body as on its mass, and is the product of the specific heat for the mass of the body. So, the equation that allows calculating heat exchanges is:

Q = c * m * ΔT

Where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation

In this case:

Replacing:

Q= 2.44 *100 g* 38 °C

Solving:

Q=9,272 J

The energy is 9,272 J (Joules)

it is a good conductor

explanation: