Heat energy of 184 kJ is given to ice of mass 600 g at −12∘C . Specific heat of ice is 2222.3Jkg−10C−1 and latent heat of ice in 336kJ/kg−1A. Final temperature of system will be 00CB. Final temperature of system will be greater than 00CC. The final system will have a mixture of ice and water in the ratio of 5:1D. The final system will have a mixture of ice and water in the ratio of 1:5E. The final system will have water onlyChoose the correct answer from the options given below:

Q1=msΔt=0.6×2222.3×12=16000.56J≈16KJFor complete meltingQrequired =mL=0.6×336=201.6KJAll ice do not melt.Mass of ice melted =184kJ−16kJ336kJ=0.5kgFinal mixture has 0.5kg water and 0.1 kg ice at 00c

Heat energy of 184 kJ is given to ice of mass 600 g at −12∘C . Specific heat of ice is 2222.3Jkg−10C−1 and latent heat of ice in 336kJ/kg−1A. Final temperature of system will be 00CB. Final temperature of system will be greater than 00CC. The final system will have a mixture of ice and water in the ratio of 5:1D. The final system will have a mixture of ice and water in the ratio of 1:5E. The final system will have water onlyChoose the correct answer from the options given below:

Q1=msΔt=0.6×2222.3×12=16000.56J≈16KJFor complete meltingQrequired =mL=0.6×336=201.6KJAll ice do not melt.Mass of ice melted =184kJ−16kJ336kJ=0.5kgFinal mixture has 0.5kg water and 0.1 kg ice at 00c

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Heat energy of 184 kJ is given to ice of mass 600 g at $- 12^{\circ} C$ . Specific heat of ice is $2222.3 J {kg}^{- 1^{0}} C^{- 1}$ and latent heat of ice in $336 kJ / {kg}^{- 1}$
A. Final temperature of system will be 0⁰C
B. Final temperature of system will be greater than 0⁰C
C. The final system will have a mixture of ice and water in the ratio of 5:1
D. The final system will have a mixture of ice and water in the ratio of 1:5
E. The final system will have water only
Choose the correct answer from the options given below:

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B and D only

A and D only

A and C only

A and E only

answer is D.

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Detailed Solution

$\begin{array}{l} Q_{1} = msΔt = 0.6 \times 2222.3 \times 12 \\ = 16000.56 J \approx 16 KJ \end{array}$
For complete melting
$\begin{array}{l} Q_{required} = mL \\ = 0.6 \times 336 = 201.6 KJ \end{array}$
All ice do not melt.
Mass of ice melted $= \frac{184 kJ - 16 kJ}{336 kJ} = 0.5 kg$
Final mixture has 0.5kg water and 0.1 kg ice at 0⁰c