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Question 21 of 30 What quantity of heat, in kJ, is required to convert 44.0 g of ethanol ($C_2H_5OH$) at 23.0 $^\circ$C to a vapor at 78.3 $^\circ$C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g $^\circ$C; $\Delta H_{vap}$ = 39.3 kJ/mol)

          Question 21 of 30
What quantity of heat, in kJ, is required to convert 44.0 g of ethanol ($C_2H_5OH$) at 23.0 $^\circ$C to a vapor at 78.3 $^\circ$C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g $^\circ$C; $\Delta H_{vap}$ = 39.3 kJ/mol)

Question 21 of 30
What quantity of heat, in kJ, is required to convert 44.0 g of ethanol (C2H5OH) at 23.0 ^∘C to a vapor at 78.3 ^∘C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g ^∘C; Δ Hvap = 39.3 kJ/mol)

Added by Joseph B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Chareen Guzman

05/04/2023

Step 1

0°C to its boiling point, 78.3°C. The formula to calculate the heat required to raise the temperature of a substance is: q = m * c * ΔT where q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. Given: m = 44.0 g c Show more…

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Question 21 of 30 What quantity of heat, in kJ, is required to convert 44.0 g of ethanol (C2H5OH) at 23.0°C to a vapor at 78.3°C, its boiling point? The specific heat capacity of ethanol is 2.46 J/g°C and Hvap is 39.3 kJ/mol.