The enthalpy of fusion of ice is 6.02 KJ mol-1.The heat capacity of `H_2O` is 4.18 Jg-1K-1. What is the smallest number of ice cubes at `0^(@)`C,each containing one mole of `H_2O`, that are needed to cool 500g of liquid water from `20^(@)`C to 0 degree C? (nearest integer)

Chemical reactions are invariably associated with the transfter of energy either in the form of heat or light. In the laboratory, heat changes in physical and chemical processes are measured with an instrument called calorimeter. Heat change in the process is calculated as {:(q = ms DeltaT,,s ="Specific heat"),(=cDeltaT,,c ="Heat capacity"):} Heat of reaction at constant volume is measured using bomb calorimeter. q_(V) = DeltaU = Internal energy change Heat of reaction at constant pressure is measured using simple or water calorimeter. q_(p) = DeltaH q_(p) = q_(V) +P DeltaV DeltaH = DeltaU +DeltanRT The enthalpy of fusion of ice is 6.02 kJ mol^(-1) . The heat capacity of water is 4.18 J g^(-1)C^(-1) . What is the smallest number of ice cubes at 0^(@)C , each containing one molw of water, the are needed to cool 500g of liquid water from 20^(@)C to 0^(@)C ?

The heat capacity of liquid water is 75.6 J/mol K, while the enthalpy of fusion of ice is 6.0 kJ/mol. What is the smallest number of ice cubes at 0^(@)C , each containing 9.0g of water, needed to cool 500g of liquid water from 20^(@)C " to " 0^(@0C ?

The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0°C is ?

Latent heat of fusion of ice is 0.333 kJ g^(-1) . The increase in entropy when 1 mole water melts at 0^(@)C will be

The enthalpy of fusion of water is 1.435kcal//mol .The molar entropy change for the melting of ice at 0^(@)C is

What is the entropy change (in JK^(-1)mol^(-1) ) when one mole of ice is converted into water at 0^(@)C ? (The enthalpy change for the conversion of ice to liquid water is 6.0KJmol^(-1) at 0^(@)C )

What is the entropy change (in JK^(-1) mol^(-1)) when one mole of ice is converted into water at 0^(@)C ? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol^(-1) at 0^(@)C )

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

How many grams of ice at 0^@C can be melted by the addition of 500 J of heat ? (The molar heat of fusion for ice is 6.02 Kamal^(-1))

4 g of O_2 and 2g of H_2 are confined in a vessel of capacity 1 litre at 0^@C . Calculate the number of moles of each gas