Calculate Δr G for the reaction at 27° C H 2( g )+2 Ag +( aq ) leftharpoons 2 A ( s )+2 H + text (aq) Given: P H 2=0.5 bar; [ Ag +]=10-5 M; [ H +]=10-3 M ; Δ G°[ Ag +( aq )]=77.1 kJ / mol

Question

Calculate Δr G for the reaction at 27° C H 2( g )+2 Ag +( aq ) leftharpoons 2 A ( s )+2 H + text (aq) Given: P H 2=0.5 bar; [ Ag +]=10-5 M; [ H +]=10-3 M ; Δ G°[ Ag +( aq )]=77.1 kJ / mol (A) -154.2 kJ / mol (B) -178.9 kJ / mol (C) -129.5 kJ / mol (D) None of these

Tardigrade Admin · Accepted Answer

Δr G°=Δ Gf (Products) -Δ Gf (Reactants) =0-77.1 × 2=-154.2 kJ / mol Q=([ H +]2/R H 2 ⋅[ Ag +]2)=(10-6/0.5 ×(10-10))=2 × 104 Δn G=Δr G°+R T ln Q Δr G=-154.2+(8.314 × 300 ln (2 × 104)/1000)=-129.5 kJ / mol

Q. Calculate $Δ_{r} G$ for the reaction at $2 7^{\circ} C$
$H_{2} (g) + 2 A g^{+} (a q) ⇌ 2 A (s) + 2 H^{+} (aq)$
Given : $P_{H_{2}} = 0.5$ bar; $[A g^{+}] = 1 0^{- 5} M$ ;
$[H^{+}] = 1 0^{- 3} M; Δ G^{\circ} [A g^{+} (a q)] = 77.1 k J / m o l$

$- 154.2 k J / m o l$

$- 178.9 k J / m o l$

$- 129.5 k J / m o l$

None of these

Q. Calculate Δr​G for the reaction at 27∘C H2​(g)+2Ag+(aq)⇌2A(s)+2H+(aq) Given : PH2​​=0.5 bar; [Ag+]=10−5M; [H+]=10−3M;ΔG∘[Ag+(aq)]=77.1kJ/mol

−154.2kJ/mol

−178.9kJ/mol

−129.5kJ/mol

None of these

Δr​G∘=ΔGf​ (Products) −ΔGf​ (Reactants) =0−77.1×2=−154.2kJ/mol Q=RH2​​⋅[Ag+]2[H+]2​=0.5×(10−10)10−6​=2×104 Δn​G=Δr​G∘+RTlnQ Δr​G=−154.2+10008.314×300ln(2×104)​=−129.5kJ/mol

Q. Calculate $Δ_{r} G$ for the reaction at $2 7^{\circ} C$
$H_{2} (g) + 2 A g^{+} (a q) ⇌ 2 A (s) + 2 H^{+} (aq)$
Given : $P_{H_{2}} = 0.5$ bar; $[A g^{+}] = 1 0^{- 5} M$ ;
$[H^{+}] = 1 0^{- 3} M; Δ G^{\circ} [A g^{+} (a q)] = 77.1 k J / m o l$

$- 154.2 k J / m o l$

$- 178.9 k J / m o l$

$- 129.5 k J / m o l$