TS EAMCET · Physics · Thermal Properties of Matter
A glass beaker contains \(200 \mathrm{~g}\) of carbonated water initially at \(20^{\circ} \mathrm{C}\). How much ice should be added to obtain the final temperature of \(0^{\circ} \mathrm{C}\) with all ice melted, if the initial temperature of ice is \(-10^{\circ} \mathrm{C}\). Neglect heat capacity of glass. [Take, \(C_{\text {water }}=4190 \mathrm{~J} / \mathrm{kg}^{\circ} \mathrm{C}\), \[ C_{\text {ice }}=2100 \mathrm{~J} / \mathrm{kg}^{\circ} \mathrm{C}, L_F=3.34 \times 10^5 \mathrm{~J} / \mathrm{kg} \text { ] } \]
- A \(47 \mathrm{~g}\)
- B \(76 \mathrm{~g}\)
- C \(200 \mathrm{~g}\)
- D \(22 \mathrm{~g}\)
Answer & Solution
Correct Answer
(A) \(47 \mathrm{~g}\)
Step-by-step Solution
Detailed explanation
Heat lost by carbonated water \(=\) Heat gained by ice Let, \(m_{\hat{i}}=\) mass of ice melted and \(m_w=\) initial mass of carbonated water.…
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