A 32-g chunk of chilled glass at 12°C is dropped into 54 g of water at 37°C. What is the equilibrium temperature of the system? The specific heats of glass and water are 0.840 a…

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asked May 28, 2020 138k views

2 Answers

Larsivi · Answer 1 · 2020-05-31T19:30:09+0000

Answer: The equilibrium temperature of the system is 29.9°C

Step-by-step explanation:

When chilled glass is dropped in water, the amount of heat released by water will be equal to the amount of heat absorbed by glass.

$Heat_{\text{absorbed}}=Heat_{\text{released}}$

The equation used to calculate heat released or absorbed follows:

$Q=m* c* \Delta T=m* c* (T_(final)-T_(initial))$

m_1* c_1* (T_(final)-T_1)=-[m_2* c_2* (T_(final)-T_2)] ......(1)

where,

q = heat absorbed or released

m_1 = mass of glass = 32 g

m_2 = mass of water = 54 g

T_(final) = final temperature = ? °C

T_1 = initial temperature of glass = 12°C

T_2 = initial temperature of water = 37°C

c_1 = specific heat of glass = 0.840 J/g°C

c_2 = specific heat of water= 4.186 J/g°C

Putting values in equation 1, we get:

32* 0.840* (T_(final)-12)=-[54* 4.186* (T_(final)-32)]

T_(final)=29.9^oC

Hence, the equilibrium temperature of the system is 29.9°C