# If the temperature of 34.4 g of ethanol increases from 25 °C to 78.8 °C, how much heat has been absorbed by the ethanol? The specific heat of ethanol is 2.44 J/(gC)?

Jun 6, 2017

The ethanol has absorbed $\text{4500 J}$.

#### Explanation:

Use the following formula:

$q = m c \Delta t$,

where $q$ is energy in Joules, $m$ is mass, $c$ is specific heat capacity, and $\Delta t$ is change in temperature: $\Delta t = \left({T}_{\text{final"-T_"initial}}\right)$

Known

$m = \text{34.4 g}$

$c = \left(\text{2.44 J")/("g"*"C"^@}\right)$

${T}_{\text{initial"="25"^@"C}}$

${T}_{\text{final"="78.8"^@"C}}$

$\Delta t = {78.8}^{\circ} \text{C"-25^@"C"="54"^@"C}$

Unknown

$q$

Insert you data into the formula and solve.

q=(34.4color(red)cancel(color(black)("g")))xx((2.44"J")/(color(red)cancel(color(black)("g"))*""^@color(red)cancel(color(black)("C"))))xx(54^@color(red)cancel(color(black)("C")))="4500 J" (rounded to two significant figures)