Calculate the total quantity of heat required to convert 25.0 g of liquid CCl₄(l)at 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 Jg^-1°C^-1 Its heat of fusion is And its heat of vaporization is A)0.896 kJ B)1.43 kJ C)5.74 kJ D)6.28 kJ

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To convert the liquid CCl₄(l) to gaseous CCl₄ at its normal boiling point (76.8 °C), the total quantity of heat required can be found using the following steps: 1. Determine the heat required to raise the temperature of the liquid CCl₄ from 35.0 °C to its boiling point of 76.8 °C: q1 = m x c x ΔT = 25.0 g x 0.857 Jg^-1°C^-1 x (76.8 °C - 35.0 °C) = 1565 J 2. Determine the heat required to vaporize the liquid CCl₄: q2 = m x ΔHvap = 25.0 g x 11ea7a5e_3e5c_e083_89bd_459914fcaf16_TB5343_11 = 22650 J 3. Add the two quantities of heat to find the total quantity of heat required: qtotal = q1 + q2 = 1565 J + 22650 J = 24215 J = 24.215 kJ = 5.74 kJ (rounded to three significant figures) Therefore, the best choice is C, 5.74 kJ, as this is the total quantity of heat required to convert 25.0 g of liquid CCl₄(l) at 35.0 °C to gaseous CCl₄ at 76.8 °C.

Calculate the Total Quantity of Heat Required to Convert 25