Calculate the total quantity of heat required to convert 25.0 g of liquid CCl₄ from 35.0°C to gaseous CCl₄ at 76.8°C (the normal boiling point for CCl₄).The specific heat of CCl₄(l)is 0.857 J/(g ∙ °C)its heat of fusion is 3.27 kJ/mol,and its heat of vaporization is 29.82 kJ/mol. A)0.896 kJ B)1.43 kJ C)5.74 kJ D)6.28 kJ

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To calculate the total heat, we need to consider both the heat required to raise the temperature of the liquid to its boiling point and the heat required to vaporize it. First, calculate the heat to raise the temperature: q1 = mass × specific heat × ΔT = 25.0 g × 0.857 J/(g∙°C) × (76.8°C - 35.0°C) = 25.0 g × 0.857 J/(g∙°C) × 41.8°C = 895.965 J = 0.896 kJ. Next, calculate the heat of vaporization: q2 = (25.0 g / 153.82 g/mol) × 29.82 kJ/mol = 4.84 kJ. Total heat = q1 + q2 = 0.896 kJ + 4.84 kJ = 5.74 kJ.

Calculate the Total Quantity of Heat Required to Convert 25