The amount of heat required to convert 1 g of ice (specific 0.5 cal at g−1oC−1 ) at −100C to steam at 100∘C is ___________.
[ Given: Latent heat of ice is 80Cal/gm, Latent heat of steam is 540Cal/gm, Specific heat of water is 1Cal/gm/C ]
725 cal
636 cal
716 cal
None of these
A
636 cal
B
716 cal
C
None of these
D
725 cal
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Solution
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Amount of heat required = Change the temp Of Ice from -10 C to 0 C + Heat required to melt the Ice + Heat required to increase the temperature of water from 0 to 100 C + Heat required to convert water at 100 C to vapor at 100 C
The amount of heat required to convert 1 g of ice (specific 0.5 cal at g−1oC−1 ) at −100C to steam at 100∘C is ___________.
[ Given: Latent heat of ice is 80Cal/gm, Latent heat of steam is 540Cal/gm, Specific heat of water is 1Cal/gm/C ]
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Q2
Ice at 0∘C is added to 1g of steam at 100∘C. For xg of ice added, the temperature of steam reduces to 0∘C. Find the value of x. (Latent heat of ice =80cal/g and latent heat of steam =540cal/g. Also, specific heat of water =1cal/ kg K)
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Q3
Work done in converting one gram of ice at −10∘C into steam at 100∘C is - [Given, specific heat of ice ci=0.5cal g−1∘C−1, specific heat of water cw=1cal g−1∘C−1, latent heat of fusion of ice Lf=80cal/g, & latent heat of vaporization of steam Lv=540cal/g]
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Q4
1g of steam at 100∘C and an equal mass of ice at 0∘C are mixed. The temperature of the mixture in steady state will be : (latent heat of steam =540cal/g, latent heat of ice =80cal/g, specific heat of water =1cal/g∘C)
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Q5
20gm ice at −10∘C is mixed with mgm steam at 100∘C. The minimum value of m so that finally all ice and steam converts into water is [ Use, specific heat and latent heat as Cice=0.5cal/gm∘C,Cwater=1cal/gm∘C,Lmelt=80cal/gm and Lvapor=540cal/gm]