369411 Calculate the change in molar Gibb's energy of carbon dioxide gas at \(\mathrm{20^{\circ} \mathrm{C}}\) when it is isothermally expanded from 1.0 to \({\rm{2}}{\rm{.0}}\,{\rm{bar}}\)

369412 Which of the following is not correct?

369413 \(\mathrm{\Delta G=-177 \mathrm{kcal}}\) for \(\mathrm{2 \mathrm{Fe}_{(s)}+\dfrac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}}\) and \(\mathrm{\Delta G=-19 \mathrm{kcal}}\) for \(\mathrm{4 \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}+\mathrm{Fe}_{(\mathrm{s})}}\) \(\mathrm{\rightarrow 3 \mathrm{Fe}_{3} \mathrm{O}_{4(\mathrm{~s})}}\)
what is the Gibb's free energy of formation of \(\mathrm{\mathrm{Fe}_{3} \mathrm{O}_{4}}\) ?

369414 Assertion :
An exothermic process, non-spontaneous at high temperature, may become spontaneous at low temperature.
Reason :
With decrease in temperature. randomness (entropy) increases.

369415 Assertion :
The thermodynamic function which determines the spontaneity of a process is the free energy. For a process to be spontaneous, the change in free energy must be negative.
Reason :
The change in free energy is related to the change in enthalpy and change in entropy. The change in entropy for a process must always be positive if it is spontaneous.

369411 Calculate the change in molar Gibb's energy of carbon dioxide gas at \(\mathrm{20^{\circ} \mathrm{C}}\) when it is isothermally expanded from 1.0 to \({\rm{2}}{\rm{.0}}\,{\rm{bar}}\)

369412 Which of the following is not correct?

369413 \(\mathrm{\Delta G=-177 \mathrm{kcal}}\) for \(\mathrm{2 \mathrm{Fe}_{(s)}+\dfrac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}}\) and \(\mathrm{\Delta G=-19 \mathrm{kcal}}\) for \(\mathrm{4 \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}+\mathrm{Fe}_{(\mathrm{s})}}\) \(\mathrm{\rightarrow 3 \mathrm{Fe}_{3} \mathrm{O}_{4(\mathrm{~s})}}\)
what is the Gibb's free energy of formation of \(\mathrm{\mathrm{Fe}_{3} \mathrm{O}_{4}}\) ?

369414 Assertion :
An exothermic process, non-spontaneous at high temperature, may become spontaneous at low temperature.
Reason :
With decrease in temperature. randomness (entropy) increases.

369415 Assertion :
The thermodynamic function which determines the spontaneity of a process is the free energy. For a process to be spontaneous, the change in free energy must be negative.
Reason :
The change in free energy is related to the change in enthalpy and change in entropy. The change in entropy for a process must always be positive if it is spontaneous.

369411 Calculate the change in molar Gibb's energy of carbon dioxide gas at \(\mathrm{20^{\circ} \mathrm{C}}\) when it is isothermally expanded from 1.0 to \({\rm{2}}{\rm{.0}}\,{\rm{bar}}\)

369412 Which of the following is not correct?

369413 \(\mathrm{\Delta G=-177 \mathrm{kcal}}\) for \(\mathrm{2 \mathrm{Fe}_{(s)}+\dfrac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}}\) and \(\mathrm{\Delta G=-19 \mathrm{kcal}}\) for \(\mathrm{4 \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}+\mathrm{Fe}_{(\mathrm{s})}}\) \(\mathrm{\rightarrow 3 \mathrm{Fe}_{3} \mathrm{O}_{4(\mathrm{~s})}}\)
what is the Gibb's free energy of formation of \(\mathrm{\mathrm{Fe}_{3} \mathrm{O}_{4}}\) ?

369414 Assertion :
An exothermic process, non-spontaneous at high temperature, may become spontaneous at low temperature.
Reason :
With decrease in temperature. randomness (entropy) increases.

369415 Assertion :
The thermodynamic function which determines the spontaneity of a process is the free energy. For a process to be spontaneous, the change in free energy must be negative.
Reason :
The change in free energy is related to the change in enthalpy and change in entropy. The change in entropy for a process must always be positive if it is spontaneous.

369411 Calculate the change in molar Gibb's energy of carbon dioxide gas at \(\mathrm{20^{\circ} \mathrm{C}}\) when it is isothermally expanded from 1.0 to \({\rm{2}}{\rm{.0}}\,{\rm{bar}}\)

369412 Which of the following is not correct?

369413 \(\mathrm{\Delta G=-177 \mathrm{kcal}}\) for \(\mathrm{2 \mathrm{Fe}_{(s)}+\dfrac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}}\) and \(\mathrm{\Delta G=-19 \mathrm{kcal}}\) for \(\mathrm{4 \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}+\mathrm{Fe}_{(\mathrm{s})}}\) \(\mathrm{\rightarrow 3 \mathrm{Fe}_{3} \mathrm{O}_{4(\mathrm{~s})}}\)
what is the Gibb's free energy of formation of \(\mathrm{\mathrm{Fe}_{3} \mathrm{O}_{4}}\) ?

369414 Assertion :
An exothermic process, non-spontaneous at high temperature, may become spontaneous at low temperature.
Reason :
With decrease in temperature. randomness (entropy) increases.

369415 Assertion :
The thermodynamic function which determines the spontaneity of a process is the free energy. For a process to be spontaneous, the change in free energy must be negative.
Reason :
The change in free energy is related to the change in enthalpy and change in entropy. The change in entropy for a process must always be positive if it is spontaneous.

369411 Calculate the change in molar Gibb's energy of carbon dioxide gas at \(\mathrm{20^{\circ} \mathrm{C}}\) when it is isothermally expanded from 1.0 to \({\rm{2}}{\rm{.0}}\,{\rm{bar}}\)

369412 Which of the following is not correct?

369413 \(\mathrm{\Delta G=-177 \mathrm{kcal}}\) for \(\mathrm{2 \mathrm{Fe}_{(s)}+\dfrac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}}\) and \(\mathrm{\Delta G=-19 \mathrm{kcal}}\) for \(\mathrm{4 \mathrm{Fe}_{2} \mathrm{O}_{3(\mathrm{~s})}+\mathrm{Fe}_{(\mathrm{s})}}\) \(\mathrm{\rightarrow 3 \mathrm{Fe}_{3} \mathrm{O}_{4(\mathrm{~s})}}\)
what is the Gibb's free energy of formation of \(\mathrm{\mathrm{Fe}_{3} \mathrm{O}_{4}}\) ?

369414 Assertion :
An exothermic process, non-spontaneous at high temperature, may become spontaneous at low temperature.
Reason :
With decrease in temperature. randomness (entropy) increases.

369415 Assertion :
The thermodynamic function which determines the spontaneity of a process is the free energy. For a process to be spontaneous, the change in free energy must be negative.
Reason :
The change in free energy is related to the change in enthalpy and change in entropy. The change in entropy for a process must always be positive if it is spontaneous.