Question

Calculate the amount of heat needed to melt 103.g of solid acetic acid (HCH3CO2) and bring it to a temperature of 62.0°C. Be sure your answer has a unit symbol and the correct number of significant digits.

Answer 1

Mass of solid acetic acid = 103 g Molar mass of acetic acid (CH,COOH) = 60.05g/mol Final temperature is to bring it = 62 °C Heat capacity for acetic acid = 2.06 J/g °C Melting point of acetic acid = 16.64 °C Enthalpy of fusion for acetic acid = 11.73 kJ/mol • Calculate the number of moles of acetic acid as shown below: 1.715 mol • Calculate the heat required for the conversion of solid acetic acid into liquid acetic acid at 16.64 °C. Enthalpy of fusion for acetic acid = 11.73 kJ/mol 9. = nx AH, ...... (1) Here, q, is the heat, n is the number of moles and AH is the molar heat of fusion. Substitute the corresponding values in equation (1): 91 = nx AH 91 = 1.715 201 x11.73 km mot 41 = 20.1169 kJ • Calculate the amount of heat required to raise the temperature of the liquid acetic acid to 62°C. 92 = mxcXAT ...... (2) Here, q, is the heat, m is the mass of the substance, AT is the change in temperature. 92 = mxcxAT 92 = 103 gx2.067 *x(62 – 16.4)% 92 = 9,675.408J 92 = 9.6754 kJ • Add q, and 92 to calculate the amount of heat needed to melt 103.g of solid acetic acid (HCH3C02) and bring it to a temperature of 62.0°C. Total heat energy required = 92 +92 = 20.1169 kJ +9.6754 kJ = 29.7923kJ =29.8 kJ