Question

1. 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/(g*°c)

Explanation:

Step1: Calculate the temperature change

$\Delta T=T_{final}-T_{initial}=78.8^{\circ}C - 25^{\circ}C=53.8^{\circ}C$

Step2: Use the heat - absorption formula

The formula for heat absorption is $q = mc\Delta T$, where $m$ is the mass, $c$ is the specific heat capacity, and $\Delta T$ is the temperature change.
Given $m = 34.4g$, $c=2.44J/(g\cdot^{\circ}C)$, and $\Delta T = 53.8^{\circ}C$
$q=(34.4g)\times(2.44J/(g\cdot^{\circ}C))\times(53.8^{\circ}C)$
First, calculate $34.4\times2.44 = 83.936$
Then, $83.936\times53.8=4515.7568J$

Answer:

$4516J$ (rounded to four significant figures)