Use tabulated half-cell potentials to calculate ΔG∘rxn for each of the following reactions at 25 ∘C....

Use tabulated half-cell potentials to calculate ΔG∘rxn for each of the following reactions at 25 ∘C.

Part A 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) Express the energy change in kilojoules to two significant figures.

Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq) Express the energy change in kilojoules to one significant figure.

Part C Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express the energy change in kilojoules to two significant figures.

Expert Solution

queen_honey_blossom answered 2 years ago

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether...

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?2CH4(g)→C2H6(g)+H2(g), Calculate ΔS∘rxn at 25 ∘C. 2NH3(g)→N2H4(g)+H2(g) Calculate ΔS∘rxn at 25 ∘C. N2(g)+O2(g)→2NO(g) Calculate ΔS∘rxn at 25 ∘C. 2KClO3(s)→2KCl(s)+3O2(g) Calculate ΔS∘rxn at 25 ∘C.

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or...

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C? a) 2CH4(g)→C2H6(g)+H2(g) b) 2NH3(g)→N2H4(g)+H2(g) c) N2(g)+O2(g)→2NO(g) d) 2KClO3(s)→2KCl(s)+3O2(g) Can you please show equations. I am having so much trouble with these.

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced...

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)

Calculate ΔG∘rxn and K for each of the following reactions. Part A The reaction of Cr3+(aq)...

Calculate ΔG∘rxn and K for each of the following reactions. Part A The reaction of Cr3+(aq) and Cr(s) to form Cr2+(aq). [The reduction potential of Cr2+(aq) to Cr(s) is -0.91 V.] Calculate ΔG∘rxn.

Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25...

Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 Part A 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) Express your answer using two significant figures. Part B O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) Express your answer using two significant figures. Part C Br2(l)+2I−(aq)→2Br−(aq)+I2(s) Express your answer using two significant figures.

1)For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. 3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g) N2(g)+3H2(g)→2NH3(g)...

1)For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. 3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g) N2(g)+3H2(g)→2NH3(g) 2)Before investigating the scene, the technician must dilute the luminol solution to a concentration of 6.00×10−2M . The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted spray? 3)A student placed 11.0 g of glucose (C6H12O6) in a volumetric flask, added enough water to dissolve...

Use the following half-reactions to write three spontaneous reactions, and calculate E cell for each reaction:...

Use the following half-reactions to write three spontaneous reactions, and calculate E cell for each reaction: a. Au+ (aq) + e- ----> Au (s) E= 1.69 V b. N2O (g) + 2H+ (aq) + 2 e- ----> N2 (g) + H2O (l) E= 1.77 V c. Cr3+ (aq) + 3e- ---> Cr (s) E= -0.74 V

Using standard electrode potentials calculate ΔG∘rxn and use its value to estimate the equilibrium constant for...

Using standard electrode potentials calculate ΔG∘rxn and use its value to estimate the equilibrium constant for each of the reactions at 25 ∘C. A. Cu2+(aq)+Zn(s)→Cu(s)+Zn2+(aq) B. Br2(l)+2Cl−(aq)→2Br−(aq)+Cl2(g) C. MnO2(s)+4H+(aq)+Cu(s)→Mn2+(aq)+2H2O(l)+Cu2+(aq) Find K. All answers must have one significant figure. Please show all your work and equations used. Thank you!!

For each of the following reactions, calculate ΔH∘rxnΔHrxn∘, ΔS∘rxnΔSrxn∘, and ΔG∘rxnΔGrxn∘ at 25 ∘C∘C. State whether...

For each of the following reactions, calculate ΔH∘rxnΔHrxn∘, ΔS∘rxnΔSrxn∘, and ΔG∘rxnΔGrxn∘ at 25 ∘C∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C∘C? Part A 2CH4(g)→C2H6(g)+H2(g)2CH4(g)→C2H6(g)+H2(g) Express your answer to one decimal place. Part B Calculate ΔS∘rxnΔSrxn∘ at 25 ∘C∘C. Express your answer to one decimal place. Part D 2NH3(g)→N2H4(g)+H2(g)2NH3(g)→N2H4(g)+H2(g) Express your answer to one...

Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following...

Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following reactions. 1. CoO(s)+H2(g)→Co(s)+H2O(g) 2. NH4I(s)→HI(g)+NH3(g) 3.H2(g)+FeO(s)→Fe(s)+H2O(g) 4.SiH4(g)→Si(s)+2H2(g)

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