I)Heat of fusion of ice at 0°C and 1atmosphere is 6.01 kJ mol" and he

1.	I)Heat of fusion of ice at 0°C and 1atmosphere is 6.01 kJ mol" and heat ofevaporation of water at 100 °C is 40.7 kJmol-1. Calculate the enthalpy change forthe conversion of 1 mole of ice at 0°C intovapour at 100°C. Heat capacity of wateris 4.184 JK-1 mol1.
Answer» Answer: heat RELEASED to cool 500g water from 20 ∘ C to 0 ∘ C. q=msΔT =500×4.18×20=41800J =41.8kJ Number of MOLES of water(ICE) that will melt to absorb 41.8kJ= 6.02 41.8 =≈7.

I)Heat of fusion of ice at 0°C and 1atmosphere is 6.01 kJ mol" and heat ofevaporation of water at 100 °C is 40.7 kJmol-1. Calculate the enthalpy change forthe conversion of 1 mole of ice at 0°C intovapour at 100°C. Heat capacity of wateris 4.184 JK-1 mol1.

Answer»

Answer:

heat RELEASED to cool 500g water from 20

∘

C to 0

∘

q=msΔT

=500×4.18×20=41800J

=41.8kJ

Number of MOLES of water(ICE) that will melt to absorb 41.8kJ=

6.02

41.8

=≈7.

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I)Heat of fusion of ice at 0°C and 1atmosphere is 6.01 kJ mol" and heat ofevaporation of water at 100 °C is 40.7 kJmol-1. Calculate the enthalpy change forthe conversion of 1 mole of ice at 0°C intovapour at 100°C. Heat capacity of wateris 4.184 JK-1 mol1.​

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I)Heat of fusion of ice at 0°C and 1atmosphere is 6.01 kJ mol" and heat ofevaporation of water at 100 °C is 40.7 kJmol-1. Calculate the enthalpy change forthe conversion of 1 mole of ice at 0°C intovapour at 100°C. Heat capacity of wateris 4.184 JK-1 mol1.