The melting point of ice is .......... Kelvin. [273 / 373]

Melting of ice into water is a

(i) Calculate the change in entropy for the fusion of 1 mole of ice. The melting point of ice is 273 K and molar enthalpy of fusion for ice = 6.0 kJ/mole. (ii) Calculate the standard of entropy change for the following reaction. {:(,H^(+)(aq), + OH(aq)to, H_(2)O(l)),(S^(@)(298 K)//JK^(-1)mol^(-1),0,-10.7,+70):}

IF the melting point of ice is 273 K and molar enthalpy of usion for ice = 6.0 kJ mol^(-1) , the change in entropy for the fusion of 1 mole of ice will be

Calculate the change in entropy for the fusion of 1 mol of ice. The melting point of ice is 300K and molar enthalpy of fustion for ice = 6.0 k J mol^(-1) .

Assertion : The melting point of ice decreases with increase of pressure Reason : Ice contract on melting.

The difference between the freezing point and the boiling point of water in the Kelvin scale is ................... (100 equal parts/273 equal parts).

Calculate the change in entropy for the fusion of 1 mole of ice (water). The melting point of water is 273 K and molar enthalpy of funsion for water =6.0 kJ mol^(-1)

Each question contains STATEMENT-1 (Assertion) and STATEMENT-2( Reason). Examine the statements carefully and mark the correct answer according to the instruction given below: STATEMENT-1: The melting point of ice decreases with increase of pressure. STATEMENT-2: Ice contracts on melting .

The triple point of water is a standard fixed point in the modern thermometry, why? What is wrong in taking the melting point of ice and boiling point of water as standard fixed point?