Question

PLEASE HELP ASAPPP

A 16.6 g sample of alcohol absorbs 890 Joules of energy as it is heated. If the initial temperature of the alcohol was
21.5 °C, what is the final temperature of the ethanol?

Answer 1

`43.2^(\circ)C`

Step-by-step explanation:

The change in temperature of the sample of alcohol is given by:

`\Delta T=(Q)/(mC_s)`

where

Q = 890 J is the amount of heat provided to the sample

m = 16.6 g is the mass of the sample

`C_s = 2.47 J/gC` is the specific heat of alcohol

Solving the equation,

`\Delta T = (890 J)/((16.6 g)(2.47 J/gC))=21.7^(\circ)C`

And since the initial temperature was

`T_i = 21.5^(\circ)C`

the final temperature is

`T_f = T_i + \Delta T=21.5^(\circ)C + 21.7^(\circ)C=43.2^(\circ)C`