1 kg of iron at $100^{o} C$ can melt more ice than 1 Kg of copper at same temperature. Explain . $(I r o n = 0.117 c a l g^{- 1}^{o} C^{- 1}; s_{c o p p e r} = 0.093 c a l g^{- 1}^{o} C^{- 1})$ .

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Solution

Ice melted depends on the amount of heat that can be delivered to ice during the reduction of the temperature of the metal from $100^{o} C$ to the temperature of ice ( $0^{o} C$ ).
$A m o u n t o f h e a t d e l i v e r e d t o i c e = a m o u n t o f l o s t b y t h e m e t a l = Q = m s Δ t$
$= m s (100 - 0) = m s \times 100$
Amount of heat lost by the metal $\propto$ s
( $∴$ mass and temperature is same for both metals)
$∴$ Amount of ice melted $\propto$ s
$S p e c i f i c h e a t o f c o p p e r = 0.093 c a l g^{- 1}^{o} C^{- 1}$
$= 390 J k g^{- 1} K^{- 1}$
$S p e c i f i c h e a t o f i r o n = 0.117 c a l g^{- 1}^{o} C^{- 1}$
$= 491 J k g^{- 1} K^{- 1}$
As 's' is more for iron, more amount of heat is lost by it and it melts more amount of ice

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100^{o}

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