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Standard X

Physics

Heating Curve of Ice

90g of water ...

Question

90g of water spilled out from a vessel in the room on the floor . assume that water vapour behaving as an ideal gas, calculate the internal energy change when the spilled water undergoes complete evaporation at 100^° C( molar heat of water=41K J mol∧1

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90 g

of water spilled out from a vessel in the room on the floor. Assuming that water vapour behaving as an ideal gas, Calculate the internal energy change when the spilled water undergoes complete evaporation at

100^{o} C

. (Given the molar enthalpy of vaporisation of water at 1 bar and

373 k = 41 k J / m o l^{- 1}

Q. For water

Δ_{v a p} H = 41 k J {mol}^{- 1}

373 K

and 1 bar pressure. Assuming that water vapour is an ideal gas the that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is ___

k J {mol}^{- 1}

.
[Use :

R = 8.3 J {mol}^{- 1} K^{- 1}

]

If water vapour is assumed to be a perfect gas, molar enthalpy change for vapourization of 1 mol of water at 1 bar and

100^{0} C

41 k J . {m o l}^{- 1}

. Calculate the internal energy change, when 1 mol of water is vaporized at 1 bar pressure and

100^{0} C

Assuming that water vapour is an ideal gas, the internal energy change $(Δ U)$ when 1 mol of water is vapourised at 1 bar pressure and 100 $^{0}$ C will be:

[Given molar enthalpy of vapourisation of water at 1bar and 373 K=41 kJ mol $^{- 1}$ ]

Q. Assuming that water vapour is an ideal gas, the internal energy change

(Δ U)

when

1

mol of water is vaporized at

1

bar pressure and

100^{o}

C (given: molar enthalpy of vaporization of water

41

k J

m o l^{- 1}

1

bar and

373

K and

R = 8.3

m o l^{- 1}

m o l^{- 1}

) will be:

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