2 kg of ice at -15°C is mixed with 5 kg of water at 40°C. c w = 4200 , c ice = 2100 J / ( kg K ) , L f = 3.36 × 1 0 5 J / kg . Find the final temperature in ∘ C . Choose the correct value.

Water to 0°C releases 840000 J. Ice needs 2 ( 2100 ) ( 15 ) + 2 ( 336000 ) = 735000 J . Spare 105000 J heats 7 kg : Δ T = 7 ( 4200 ) 105000 = 3.5 7 ∘ C . All ice melts; final 3.57°C. Option D.

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Physics - Heat & Thermo Question with Solution | TestHub

PhysicsHeat & ThermoThermal ExpansionMedium2 minQB

PhysicsMediumsingle choice

2 kg of ice at -15°C is mixed with 5 kg of water at 40°C. $c_{w} = 4200, c_{ice} = 2100 J / (kg K), L_{f} = 3.36 \times 1 0^{5}$ $J / kg$ . Find the final temperature in $^{\circ} C$ . Choose the correct value.

Options:

Answer:

Solution:

Water to 0°C releases 840000 J. Ice needs $2 (2100) (15) + 2 (336000) = 735000 J$ . Spare 105000 J heats $7 kg : Δ T = \frac{105000}{7 ( 4200 )} = 3.5 7^{\circ} C$ . All ice melts; final 3.57°C. Option D.

Subject:PhysicsTopic:Heat & ThermoSubtopic:Thermal Expansion

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