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Which quantity out of Delta(r)G " and " ...

Which quantity out of `Delta_(r)G " and " Delta_(r) G^(Θ)` will be zero at equilibrium ?

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To determine which quantity, \( \Delta_r G \) or \( \Delta_r G^\circ \), will be zero at equilibrium, we can follow these steps: ### Step-by-Step Solution: 1. **Understand the Terms**: - \( \Delta_r G \) represents the change in Gibbs free energy for a reaction under non-standard conditions. - \( \Delta_r G^\circ \) represents the change in Gibbs free energy for a reaction under standard conditions. ...
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(a) A sample of 1.0 mol of a monoatomic ideal gas is taken through a cyclic process of expansion and compression as shown in figure. What will be the value of DeltaH for the cycle as a whole? (b) Which quantity out of Delta_(r)G and Delta_(r)G^(Theta) will be zero at equilibrium?

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )H^(@) at 320 K is :

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )H^(@) at 300 K for the reaction is :

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )S^(@) at 320 K is :

Standard Gibb's energy of reaction (Delta_(r )G^(@)) at a certain temperature can be computed Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r )S^(@) and the change in the value of Delta_(r)H^(@) and Delta_(r)S^(@) for a reaction with temperature can be computed as follows : Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)(T_(2)-T_(1)) Delta_(r )S_(T_(2))^(@)-Delta_(r )S_(T_(1))^(@)=Delta_(r )C_(p)^(@)ln.(T_(2)/T_(1)) " "Delta_(r )G^(@)=Delta_(r)H^(@)-T.Delta_(r)S^(@) and " by "Delta_(r )G^(@)=-"RT " ln K_(eq) . Consider the following reaction : CO(g)+2H_(2)(g)iffCH_(3)OH(g) Given : Delta_(f)H^(@)(CH_(3)OH,g)=-201 " kJ"//"mol", " "Delta_(f)H^(@)(CO,g)=-114" kJ"//"mol" S^(@)(CH_(3)OH,g)=240" J"//"K-mol, "S^(@)(H_(2),g)=29" JK"^(-1)" mol"^(-1) S^(@)(CO,g)=198 " J"//"mol-K, "C_(p,m)^(@)(H_(2))=28.8 " J"//"mol-K" C_(p,m)^(@)(CO)=29.4 " J"//"mol-K, "C_(p,m)^(@)(CH_(3)OH)=44 " J"//"mol-K" and " "ln ((320)/(300))=0.06 , all data at 300 K Delta_(r )S^(@) at 300 K for the reaction is :

Variation of equilibrium constan K with temperature is given by van't Hoff equation InK=(Delta_(r)S^(@))/R-(Delta_(r)H^(@))/(RT) for this equation, (Delta_(r)H^(@)) can be evaluated if equilibrium constants K_(1) and K_(2) at two temperature T_(1) and T_(2) are known. log(K_(2)/K_(1))=(Delta_(r)H^(@))/(2.303R)[1/T_(1)-1/T_(2)] For an isomerization X(g)hArrY(g) the temperature dependency of equilibrium constant is given by : lnK=2-(1000)/T The value of Delta_(r)S^(@) at 300 K is :

Variation of equilibrium constan K with temperature is given by van't Hoff equation InK=(Delta_(r)S^(@))/R-(Delta_(r)H^(@))/(RT) for this equation, (Delta_(r)H^(@)) can be evaluated if equilibrium constans K_(1) and K_(2) at two temperature T_(1) and T_(2) are known. log(K_(2)/K_(1))=(Delta_(r)H^(@))/(2.303R)[1/T_(1)-1/T_(2)] Select the correct statement :

Enthalpy is an extensive property. In general, if enthalpy of an overall reaction A rarr B along one route is Delta_(r) H " and Delta_(r) H_(1), Delta_(r) H_(2), Delta_(r) H_(3) ..... Represent enthalpies of intermediate reactions leading to product B. What will be the relation between Delta_(r)H overall reaction and Delta_(r)H_(1), Delta_(r)H_(2) ... etc for intermediate reaction.

Standard molar enthalpy of formation, Delta_(f) H^(Θ) is just a special case of enthalpy of reaction, Delta_(r) H^(Θ) . Is the Delta_(r) H^(Θ) same as standard molar enthalpy of formation ? Given reason for your answer. CaO (s) + CO_(2) (g) rarr CaCO_(3) (s) , Delta_(f) H^(Θ) = - 178.3 kJ mol^(-1)

For the reaction at 298K: A_((g)) +B_((g)) hArr C_((g)) + D_((g)) Delta H^(@) + 29.8kcal and Delta S^(@) = 100cal K^(-1) . Find the value of equilibrium constant.

NCERT EXEMPLAR ENGLISH-THERMODYNAMICS-Multiple choice questions
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  2. The molar enthalpy of vaporisation of acetone is less than that of wat...

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  3. Which quantity out of Delta(r)G " and " Delta(r) G^(Θ) will be zero at...

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  9. If the combustion of 1 g of graphite produces -20.7 kJ of heat, what w...

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  13. What will be the work done on an ideal gas enclosed in a cyliner, when...

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  14. How will you calculate work done on an ideal gas in a compression, whe...

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  15. Represent the potential energy/enthalpy change in the following proces...

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  16. Enthalpy diagram for a particular reaction is given in figure. Is it p...

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  17. 1.0 mol of a monoatomic ideal gas is expanded from state (1) to state ...

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  18. An ideal gas is allowed to expand against a constant pressure of 2 bar...

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