273052 Given below are two statements:
Statement I: According to the Ellingham diagram, any metal oxide with higher $\Delta \mathrm{G}^{\circ}$ is more stable than the one with lower $\Delta \mathrm{G}^{\circ}$
Statement II: The metal involved in the formation of oxide placed lower in the Ellingham diagram can reduce the oxide of a metal placed higher in the diagram.
In the light of the above statements, choose the most appropriate answer from the options given below:

273055 An endothermic reaction is found to have +ve entropy change. The reaction will be

273058 Following reaction occurrs in an automobile
$2 \mathrm{C}_8 \mathrm{H}_{18}(\mathrm{~g})+25 \mathrm{O}_2(\mathrm{~g}) \rightarrow 16 \mathrm{CO}_2(\mathrm{~g})+18 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$
The sign of $\Delta H, \Delta S$ and $\Delta G$ would be

273059 For a reaction to be spontaneous at all temperatures,

273052 Given below are two statements:
Statement I: According to the Ellingham diagram, any metal oxide with higher $\Delta \mathrm{G}^{\circ}$ is more stable than the one with lower $\Delta \mathrm{G}^{\circ}$
Statement II: The metal involved in the formation of oxide placed lower in the Ellingham diagram can reduce the oxide of a metal placed higher in the diagram.
In the light of the above statements, choose the most appropriate answer from the options given below:

273055 An endothermic reaction is found to have +ve entropy change. The reaction will be

273058 Following reaction occurrs in an automobile
$2 \mathrm{C}_8 \mathrm{H}_{18}(\mathrm{~g})+25 \mathrm{O}_2(\mathrm{~g}) \rightarrow 16 \mathrm{CO}_2(\mathrm{~g})+18 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$
The sign of $\Delta H, \Delta S$ and $\Delta G$ would be

273059 For a reaction to be spontaneous at all temperatures,

273052 Given below are two statements:
Statement I: According to the Ellingham diagram, any metal oxide with higher $\Delta \mathrm{G}^{\circ}$ is more stable than the one with lower $\Delta \mathrm{G}^{\circ}$
Statement II: The metal involved in the formation of oxide placed lower in the Ellingham diagram can reduce the oxide of a metal placed higher in the diagram.
In the light of the above statements, choose the most appropriate answer from the options given below:

273055 An endothermic reaction is found to have +ve entropy change. The reaction will be

273058 Following reaction occurrs in an automobile
$2 \mathrm{C}_8 \mathrm{H}_{18}(\mathrm{~g})+25 \mathrm{O}_2(\mathrm{~g}) \rightarrow 16 \mathrm{CO}_2(\mathrm{~g})+18 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$
The sign of $\Delta H, \Delta S$ and $\Delta G$ would be

273059 For a reaction to be spontaneous at all temperatures,

273052 Given below are two statements:
Statement I: According to the Ellingham diagram, any metal oxide with higher $\Delta \mathrm{G}^{\circ}$ is more stable than the one with lower $\Delta \mathrm{G}^{\circ}$
Statement II: The metal involved in the formation of oxide placed lower in the Ellingham diagram can reduce the oxide of a metal placed higher in the diagram.
In the light of the above statements, choose the most appropriate answer from the options given below:

273055 An endothermic reaction is found to have +ve entropy change. The reaction will be

273058 Following reaction occurrs in an automobile
$2 \mathrm{C}_8 \mathrm{H}_{18}(\mathrm{~g})+25 \mathrm{O}_2(\mathrm{~g}) \rightarrow 16 \mathrm{CO}_2(\mathrm{~g})+18 \mathrm{H}_2 \mathrm{O}(\mathrm{g})$
The sign of $\Delta H, \Delta S$ and $\Delta G$ would be

273059 For a reaction to be spontaneous at all temperatures,