An ice cube of mass 10 g at-10^° C is dropped into a calorimeter containing 20 g water at 20^° C . If water equivalent of calorimeter is 10 g, then finaltemperature of mixture in calorimeter would be

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10

g of ice at

- 20^{o}

C is dropped into a calorimeter containing

10

g of water at

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C; the specific heat of water is twice that of ice. When equilibrium is reached, the calorimeter will contain.

10 g of ice at $- 20^{\circ} C$ is dropped into a calorimeter containing 10 g of water at $10^{\circ} C$ ; the specific heat of water is twice that of ice. Ehen equilibrium is reached, the calorimeter will contain

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Q. 10 g of ice at

- 20^{o} C

is dropped into a calorimeter containing 10 g of water at

10^{o} C

; the specific heat of water is twice that of ice. When equilibrium is reached, the calorimeter will contain:

Q. 10 gm of ice at

- 20^{\circ} C

is dropped into a calorimeter containing 10 gm of water at

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. The specific heat of water is twice that of ice. Neglect heat capacity of the calorimeter. When equilibrium is reached, the calorimeter will contain :-

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