MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Heat Capacity

Assuming that...

Question

Assuming that water vapour is an ideal gas, the internal energy change when 1 mole of water is vaporised at 1 bar pressure and 100°C,(Given: molar enthalpy of vaporization of water at 1 bar and 373 kelvin = 41KJ mol^-1 and R= 8.3mole^-1K^-1) will be

Open in App

Solution

Suggest Corrections

thumbs-up

0

Similar questions

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

(Δ U

1

mol of water is vaporised at

1

bar pressure and

100^{o} C

, (given: molar enthalpy of vaporisation of water at

1

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

R = 8.314 J K^{- 1} {m o l}^{- 1}

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

(Δ U)

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

373

R = 8.3

m o l^{- 1}

m o l^{- 1}

Assuming that, water vapour is an ideal gas the internal energy change (ΔU)(ΔU) when 11 mol of water is vaporized at 11 bar pressure and 100o100o C will be:

[given: molar enthalpy of vaporisation of water at

1

373

= 41

m o l^{- 1}

R = 8.3

K^{- 1}

m o l^{- 1}

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

Δ U

1 m o l

of water is vaporised at

1

bar pressure and

100^{o} C

(Given: Molar enthalpy of vapourisation of water at

1

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

R = 8.3 J {m o l}^{- 1}

K^{- 1}

Assuming that water vapour is an ideal gas, the internal energy change (∆U) when 1 mol of water is vapourised at 1 bar pressure and 100 $^{\circ}$ C, (given : molar enthalpy of vapourisation of water at 1 bar and 373 K = 41 kJ mol $^{- 1}$ and R = 8.3 J mol $^{- 1}$ K $^{- 1}$ ) will be

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Thermodynamic Processes

PHYSICS

Watch in App

explore_more_icon

Explore more

Standard XII Physics

Join BYJU'S Learning Program

CrossIcon