Use the standard reduction potentials to determine the G of the reaction of Tl(s) and H(aq) to produce (a) Tl(aq) and H2(g) and (b) Tl5+(aq) and H2(g).
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Use the standard reduction potentials to determine the G of the
reaction of Tl(s) and H(aq)...
Use standard reduction potentials to determine the ∆G0 of the reaction of Tl(S) and H+(aq) to...
Use standard reduction potentials to determine the ∆G0 of the reaction of Tl(S) and H+(aq) to produce (a) Tl+(aq) and H2(g)and (b) Tl3+(aq) and H2(g). Which reaction is more thermodynamically spontaneous under standard-state conditions? Comment on the results relative to the inert-pair effect.
Using the table of standard reduction potentials, answer True or False. The reaction: 2Cu(s) + 2H+(aq)...
Using the table of standard reduction potentials, answer True or False. The reaction: 2Cu(s) + 2H+(aq) ⇋ 2Cu+(aq) + H2 (g) will occur (is spontaneous) at STP.
3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s)...
3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s) | Tl+(aq, 0.50 mol L−1) || H+(aq, x mol L−1) | H2(g, 1 atm) | Pt(s) The concentration of H+ is unknown and the pressure of H2 is kept constant at 1 atm. The cell voltage is initially measured as 0.139 V, with the Pt | H2 | H+ half-cell acting as the cathode. (a) (6 marks) Write out the oxidation and reduction half...
A. Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H+(aq) + Fe(s)...
A. Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H+(aq) + Fe(s) H2(g) + Fe2+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: _____ G° for this reaction would be _____ (greater/less) than zero. B. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd2+(aq) + 2Ag(s)Cd(s) + 2Ag+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2 (aq)-H2(g2Cu (aq) 2H...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2 (aq)-H2(g2Cu (aq) 2H (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm Equilibrium constant than zero. AG for this reaction would be 8 more group attempts remaining Retry Entire Group Submit Answer Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H (aq)+Hg) H2() + Hg2 " (aq ) Hint: Carry at least...
Given the following standard reduction potentials: Tl(3+) + e(-) ---> Tl(2+) E°= -0.37 V Tl(3+) +...
Given the following standard reduction potentials: Tl(3+) + e(-) ---> Tl(2+) E°= -0.37 V Tl(3+) + 2e(-) ---> Tl(+) E°= 1.25 V (a) Calculate the half-cell potential for the half-reaction Tl(2+) + e(-) ---> Tl(+) (b) Determine of the following disproportionate reaction will occur sponta- neously in aqueous solution in the standard condition. 2Tl(2+)(aq) ---> Tl(3+)(aq) + Tl(+)(aq)
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe2+ (aq) + H2(g)...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe2+ (aq) + H2(g) Fe(s) + 2H+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AGº for this reaction would be than zero.
29. Use the Standard Reduction Potentials table to predict whether the redox reactions below would be...
29. Use the Standard Reduction Potentials table to predict whether the redox reactions below would be spontaneous or nonspontaneous in the forward direction in 1.0 Maqueous solution 25°C. a) Snº+(ag) + Ni(s) → Ni2+(aq) + Sna+(aq) b) H2(g) + 2 OH- (aq) + Ca2+(ag) - Ca(s) + 2 H20 (1)
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq)...
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq) 1.36 O2(g)+4H+(aq)+4e? ?2H2O(l) 1.23 Br2(l)+2e? ?2Br?(aq) 1.09 NO3?(aq)+4H+(aq)+3e? ?NO(g)+2H2O(l) 0.96 Ag+(aq)+e? ?Ag(s) 0.80 I2(s)+2e? ?2I?(aq) 0.54 Cu2+(aq)+2e? ?Cu(s) 0.16 2H+(aq)+2e? ?H2(g) 0 Cr3+(aq)+3e? ?Cr(s) -0.73 2H2O(l)+2e? ?H2(g)+2OH?(aq) -0.83 Mn2+(aq)+2e? ?Mn(s) -1.18 How can the table be used to predict whether or not a metal will dissolve in HCl? In HNO3? Drag the terms on the left to the appropriate blanks on the right to...
A) Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard...
A) Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: 2Fe3+(aq) + Pb(s) ---> 2Fe2+(aq) + Pb2+(aq) Answer: ____ kJ K for this reaction would be ________ (greater/less) than one. B) The free energy change for the following reaction at 25 °C, when [Hg2+] = 1.12 M and [H+] = 6.80×10-3 M, is -178 kJ: Hg2+(1.12 M) + H2(g) ---> Hg(l) + 2H+(6.80×10-3 M) ΔG =...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2Cu2 (aq)-H2(g2Cu (aq) 2H (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm Equilibrium constant than zero. AG for this reaction would be 8 more group attempts remaining Retry Entire Group Submit Answer Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2H (aq)+Hg) H2() + Hg2 " (aq ) Hint: Carry at least...
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe2+ (aq) + H2(g) Fe(s) + 2H+ (aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AGº for this reaction would be than zero.
29. Use the Standard Reduction Potentials table to predict whether the redox reactions below would be spontaneous or nonspontaneous in the forward direction in 1.0 Maqueous solution 25°C. a) Snº+(ag) + Ni(s) → Ni2+(aq) + Sna+(aq) b) H2(g) + 2 OH- (aq) + Ca2+(ag) - Ca(s) + 2 H20 (1)
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