Question

10 kg of ice at -10°C is mixed with 40 kg of water
at 45°C. The final temperature of mixture is :
(specific heat of ice = 2100 J/kg-k)
(1) 19°C
(2) 17°C
(3) 15°C
(4) 13°C​

Answer 1

Answer:

2 is the correct ans according to me

Answer 2

Answer:

The final temperature of the mixture is 64°C. Answer (5).

Explanation:

To solve this problem we have to apply the law of conservation of energy, which states that the total energy of a closed system remains constant. This is a system of ice and water.

We must first calculate the amount of thermal energy required to melt the ice. The formula for calculating the thermal energy required to change the physical state of a substance is Q = ml, where Q is the thermal energy, m is the mass of the substance, and L is the latent heat of fusion. For ice, the value of L is 334 kJ/kg.

The thermal energy required to melt 10 kg of ice at -10°C is therefore Q = 10 x 334000 = 3340000 J.

Next we need to calculate the thermal energy extracted from the water. The formula for calculating the thermal energy gained from a substance is Q = mcΔT, where Q is the thermal energy, m is the mass of the substance, c is the specific heat and ΔT is the temperature change. For water the value of c is 4186 J/kg-K.

Therefore, the thermal energy absorbed by 40 kg of water at 45 °C is Q = 40 x 4186 x (T - 45), where T is the final temperature of the mixture.

Using the

, we can equate the heat energy gained from the water to the heat energy required to melt the ice and calculate T.

40 x 4186 x (T - 45) = 3340000

T - 45 = 19

T = 64°C

The final temperature of the mixture is 64°C. Answer (5)

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