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Standard X

Physics

Unit of Heat

A copper calo...

Question

A copper calorimeter of mass 100g contains 150g of water and 10g of ice in thermal equilibrium at atmospheric pressure. A piece of lead of mass 100g at 200°C is dropped into calorimeter . Find the final temperature (assume no heat is lost to the surrounding) and the amount of ice left. (Take L=335 kJ/kg), if required.

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https://forum.byjus.com/calculate-the-amount-of-ice-which-is-required-to-cool-150-g-of-water-contained-in-a-vessel-of-mass-100-g-at-30c-such-that-the-final-temperature-of-the-mixture-is-5oc-take-specific-heat-capacit

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Similar questions

Q. A calorimeter has mass

100 g

and specific heat

0.1 k c a l / k g^{\circ} C

. It contains

250 g m

of liquid at

30^{\circ} C

having specific heat of

0.4 k c a l / k g^{\circ} C

. If we drop a piece of ice of mass

10 g

0^{\circ} C

. What will be the temperature of the mixture?

Q. A metallic calorimeter of mass 100g contains 200 g of ice and the initial temperature of the calorimeter and the ice is

- 10^{\circ} C

. Heat is supplied to the system containing calorimeter and ice at a constant rate of

50 c a l s^{- 1}

. Find the time required to raise the temperature of the system to

50^{\circ} C

. [Neglect the loss of heat to the surroundings].

Take specific heat capacity of calorimeter and ice as

0.2 c a l g^{- 1}^{\circ} C^{- 1}

and

\frac{1}{2} c a l g^{- 1}^{\circ} C^{- 1}

.Take latent heat of fusion of ice as

80 c a l g^{- 1}

and specific heat capacity of water as

1 c a l g^{- 1}^{\circ} C^{- 1}

Q. Water of mass

m_{2} = 1 k g

is contained in a copper calorimeter of mass

m_{1} = 1 k g

. Their common temperature is

t = 10^{o} C

. Now a piece of ice of mass

m_{3} = 2 k g

and temperature

- 11^{o} C

is dropped into the calorimeter. Neglecting any heat loss, the final temperature of the system is [specific heat of copper

0.1 K c a l / k g^{o} C

, specific heat of water

= 1 K c a l / k g^{o} C

, specific heat of ice

= 0.5 K c a l / k g^{o} C

, latent heat of fusion of ice

= 78.7 K c a l / k g

]

Q. A calorimeter of mass m contains an equal mass of water in it. The temperature of the water and calorimeter is

t_{2} > 0^{\circ} C

. A block of ice of mass m and temperature

t_{3} < 0^{\circ} C

is gently dropped into the calorimeter. Let

C_{1}, C_{2}

and

C_{3}

be the specific heats of material of calorimeter, water and ice respectively and L be the Latent heat of ice. The whole mixture in the calorimeter becomes ice if

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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