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)?

Question

Jeremiah Adams · Accepted Answer

The ethanol has absorbed #"4500 J"#.

Use the following formula: #q=mcDeltat#, where #q# is energy in Joules, #m# is mass, #c# is specific heat capacity, and #Deltat# is change in temperature: #Deltat=(T_"final"-T_"initial")# Organize your data: Known #m="34.4 g"# #c=("2.44 J")/("g"*"C"^@")# #T_"initial"="25"^@"C"# #T_"final"="78.8"^@"C"# #Deltat=78.8^@"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)

Natalie Anton · Answer

undefined Use the formula Q = mcΔT, where Q is heat, m is mass, c is specific heat, and ΔT is temperature change.

$$ Q = (34.4 \, g)(2.44 \, J/(g°C))(78.8°C - 25°C) $$

$$ Q = 7162.4 \, J $$

The heat absorbed by ethanol is 7162.4 J.