From the following data, determine the enthalpy change for the sublimation of ice at 223 K [mean heat capacity of ice = 2 $J K^{- 1} g m^{- l}$ , mean heat capacity of $H_{2} O (l) = 4.2 J K^{- 1} g m^{- 1}$ , mean heat capacity of $H_{2} O (v) = 1.85 J K^{- 1} g m^{- 1}$ , enthalpy of fusion of ice at $0^{\circ} C = 6.01 K J / M O L$ .enthalpy of evaporation of water at $100^{\circ} C = 2255 J g m^{- 1}$ ]

2831.5 J . g^{- 1}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

2431.5 J . g^{- 1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2731.5 J . g^{- 1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

2881.5 J . g^{- 1}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is C $2831.5 J . g^{- 1}$
$Δ H_{f u s} + Δ H_{v a p} = Δ H_{s u b}$
$Δ H = C_{p} Δ T$
$\Delta H_{fus}=
$ \Delta H_{sub} =

Suggest Corrections

Similar questions

Q. The enthalpy of fusion of ice is

6.02 k J m o l^{- 1}

. The heat capacity of water is

4.18 J g^{- 1} C^{- 1}

. What is the smallest number of ice cubes at

0^{\circ} C

, each containing one mole of water, that are needed to cool

500 g

of liquid water from

20^{\circ} C

0^{\circ} C

Q. Calculate the amount of heat reqiured to convert

1 kg

of ice at

- 10^{\circ} C

into steam at

100^{\circ} C

. Specific heat capacity of ice is

= 2100 J {k g}^{- 1} K^{- 1}

, latent heat of fusion of ice

= 3.36 \times 10^{5} J {k g}^{- 1}

, specific heat capacity of water

= 4200 J {k g}^{- 1} K^{- 1}

and latent heat of vapourization of water

= 2.25 \times 10^{6} J {k g}^{- 1}

A 5 g piece of ice at $- 20^{\circ}$ C is put into 10 g of water at $30^{\circ}$ C. Assuming that heat is exchanged only between the ice and the water. Then find the heat required for phase change. Specific heat capacity of ice $= 2100 J k g^{- 1}^{\circ} C^{- 1}$ . Specific heat capacity of water $= 4200 J k g^{- 1}^{\circ} C^{- 1}$ and latent heat of fusion of ice $3.36 \times 10^{5} J k g^{- 1}$ .