1a. If 24.028 g of benzene, C6H6, at 9.025 °C absorbs 2.71 kJ of energy in the f

Question

1a. If 24.028 g of benzene, C6H6, at 9.025 °C absorbs 2.71 kJ of energy in the form of heat, what is the final temperature of the benzene? The specific heat capacity of benzene is 1.72 J/g×K

1b) A 24.952 g sample of metal at 74.21°C is added to 26.608 g of H2O(l) at 12.012°C in an insulated container. The temperature rises to 15.42 °C. Neglecting the heat capacity of the container, what is the specific heat capacity of the metal? The specific heat capacity of H2O(l) is 4.184 J/(g·°C)

1c) What is the difference between both temperatures in Kelvin?

Explanation / Answer

1a)

mass of benzene = 24.028 g

specific heat = 1.72 J / g oC

heat Q = 2.71 kJ = 2710 J

Q = m Cp dT

2710 = 24.028 x 1.72 x (Tf - 9.025)

Tf = 74.60 oC

final temperature = 74.60 C

b)

here heat loss by metal = heat gain by water

24.952 x Cp x (74.21 - 15.42) = 26.608 x 4.184 x (15.42 - 12.012)

Cp = 0.2586 J / (g·°C

specific heat of metal = 0.2586 J / (g·°C

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