369253 The enthalpy of fusion of water is \(\mathrm{1.435 \mathrm{kcal} /}\)mol. The molar entropy change for the melting of ice at \(\mathrm{0^{\circ} \mathrm{C}}\) is

369254 What are the signs of the entropy change (+ or - ) in the following cases.
I: A liquid crystallizes into a solid
II: Temperature of a crystalline solid is raised from 0 K to 115 K
III. \(2{\rm{NaHC}}{{\rm{O}}_3}(\;{\rm{s}}) \to \)
\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{C}}{{\rm{O}}_{\rm{3}}}({\rm{s}}) + {\rm{C}}{{\rm{O}}_{\rm{2}}}({\rm{g}}) + {{\rm{H}}_{\rm{2}}}{\rm{O}}({\rm{g}})\)
IV. \(\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})\)

369255 One mole of \(\mathrm{\mathrm{NaCl}(\mathrm{s})}\) on melting absorbed 30.5 \(\mathrm{\mathrm{kJ}}\) of heat and its entropy is increased by \(\mathrm{28.8 \mathrm{JK}^{-1}}\). The melting point of \(\mathrm{\mathrm{NaCl}}\) is

369256 Assertion :
Water in liquid state is more stable than ice at room temperature.
Reason :
Water in liquid form has higher entropy than ice.

369253 The enthalpy of fusion of water is \(\mathrm{1.435 \mathrm{kcal} /}\)mol. The molar entropy change for the melting of ice at \(\mathrm{0^{\circ} \mathrm{C}}\) is

369254 What are the signs of the entropy change (+ or - ) in the following cases.
I: A liquid crystallizes into a solid
II: Temperature of a crystalline solid is raised from 0 K to 115 K
III. \(2{\rm{NaHC}}{{\rm{O}}_3}(\;{\rm{s}}) \to \)
\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{C}}{{\rm{O}}_{\rm{3}}}({\rm{s}}) + {\rm{C}}{{\rm{O}}_{\rm{2}}}({\rm{g}}) + {{\rm{H}}_{\rm{2}}}{\rm{O}}({\rm{g}})\)
IV. \(\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})\)

369255 One mole of \(\mathrm{\mathrm{NaCl}(\mathrm{s})}\) on melting absorbed 30.5 \(\mathrm{\mathrm{kJ}}\) of heat and its entropy is increased by \(\mathrm{28.8 \mathrm{JK}^{-1}}\). The melting point of \(\mathrm{\mathrm{NaCl}}\) is

369256 Assertion :
Water in liquid state is more stable than ice at room temperature.
Reason :
Water in liquid form has higher entropy than ice.

369253 The enthalpy of fusion of water is \(\mathrm{1.435 \mathrm{kcal} /}\)mol. The molar entropy change for the melting of ice at \(\mathrm{0^{\circ} \mathrm{C}}\) is

369254 What are the signs of the entropy change (+ or - ) in the following cases.
I: A liquid crystallizes into a solid
II: Temperature of a crystalline solid is raised from 0 K to 115 K
III. \(2{\rm{NaHC}}{{\rm{O}}_3}(\;{\rm{s}}) \to \)
\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{C}}{{\rm{O}}_{\rm{3}}}({\rm{s}}) + {\rm{C}}{{\rm{O}}_{\rm{2}}}({\rm{g}}) + {{\rm{H}}_{\rm{2}}}{\rm{O}}({\rm{g}})\)
IV. \(\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})\)

369255 One mole of \(\mathrm{\mathrm{NaCl}(\mathrm{s})}\) on melting absorbed 30.5 \(\mathrm{\mathrm{kJ}}\) of heat and its entropy is increased by \(\mathrm{28.8 \mathrm{JK}^{-1}}\). The melting point of \(\mathrm{\mathrm{NaCl}}\) is

369256 Assertion :
Water in liquid state is more stable than ice at room temperature.
Reason :
Water in liquid form has higher entropy than ice.

369253 The enthalpy of fusion of water is \(\mathrm{1.435 \mathrm{kcal} /}\)mol. The molar entropy change for the melting of ice at \(\mathrm{0^{\circ} \mathrm{C}}\) is

369254 What are the signs of the entropy change (+ or - ) in the following cases.
I: A liquid crystallizes into a solid
II: Temperature of a crystalline solid is raised from 0 K to 115 K
III. \(2{\rm{NaHC}}{{\rm{O}}_3}(\;{\rm{s}}) \to \)
\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{C}}{{\rm{O}}_{\rm{3}}}({\rm{s}}) + {\rm{C}}{{\rm{O}}_{\rm{2}}}({\rm{g}}) + {{\rm{H}}_{\rm{2}}}{\rm{O}}({\rm{g}})\)
IV. \(\mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})\)

369255 One mole of \(\mathrm{\mathrm{NaCl}(\mathrm{s})}\) on melting absorbed 30.5 \(\mathrm{\mathrm{kJ}}\) of heat and its entropy is increased by \(\mathrm{28.8 \mathrm{JK}^{-1}}\). The melting point of \(\mathrm{\mathrm{NaCl}}\) is

369256 Assertion :
Water in liquid state is more stable than ice at room temperature.
Reason :
Water in liquid form has higher entropy than ice.