1. One of the half-reactions for the electrolysis of water is 2H2O(l) →O2(g) + 4H+(aq) +...

1. One of the half-reactions for the electrolysis of water is

2H₂O(l) →O₂(g) + 4H⁺(aq) + 4e⁻

If 0.992 L of O₂ is collected at 25°C and 755 mmHg, how many faradays of electricity had to pass through the solution?

2.

What is E°_cell for the following reaction?

2 Ag(s) + Sn²⁺(aq) → 2 Ag⁺(aq) + Sn(s)

Ag⁺(aq) + e^– → Ag(s)	E° = 0.80 V
Sn⁴⁺(aq) + 2e^– → Sn²⁺(aq)	E° = 0.13 V
Sn²⁺(aq) + 2e^– → Sn(s)	E° = –0.14 V

+0.94 V

–0.94 V

+0.67 V

–0.67 V

+1.34 V

3. One of the half-reactions for the electrolysis of water is

2H⁺(aq) + 2e⁻ →H₂(g)

If 0.845 L of H₂ is collected at 25°C and 782 mmHg, how many faradays of electricity had to pass through the solution?

Expert Solution

queen_honey_blossom answered 2 years ago

answer both pls 1. Consider the following half-reaction. 4H+(aq) + O2(g) + 4e- → 2H2O(l) Eo...

answer both pls 1. Consider the following half-reaction. 4H+(aq) + O2(g) + 4e- → 2H2O(l) Eo = 1.23 V What is E, if the pressure of oxygen gas is 1.0 atmosphere and the pH is 2.92? USE 2 DECIMAL PLACES. (Hint, are solids and pure liquids included in Q? Using LeChatelier's principle is E going to be larger or smaller?) 2. Mg2C2O4(s) → 2Mg2+(aq) +C2O42-(aq) Ksp = 8.6 x 10-5 What is Qsp if 100 mL of 0.080 M Mg(N03)2...

The standard half-cell potential for the reaction O2(g)+4H+(aq)+4e−→2H2O(l) is +1.229 V at 298.15 K. The aO2...

The standard half-cell potential for the reaction O2(g)+4H+(aq)+4e−→2H2O(l) is +1.229 V at 298.15 K. The aO2 = 1.00 assuming that the aH+ is equal to the molality. Part A Calculate E for a 0.100-molal solution of H2SO4 for aO2 = 1.00 assuming that the aH+ is equal to the molality. Part B Calculate E for a 0.100-molal solution of H2SO4 for aO2= 1.00 using the measured mean ionic activity coefficient for this concentration from the data tables in the textbook....

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)...

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq) D. Determine whether the reaction in part A is spontaneous as written. E. Determine whether the reaction in part B is spontaneous as written. F. Determine whether the reaction in part C is spontaneous as written.

Hydrogen peroxide, H2O2H2O2, is used to disinfect contact lenses. 2H2O2(aq)→2H2O(l)+O2(g)2H2O2(aq)→2H2O(l)+O2(g) You may want to reference (Page)...

Hydrogen peroxide, H2O2H2O2, is used to disinfect contact lenses. 2H2O2(aq)→2H2O(l)+O2(g)2H2O2(aq)→2H2O(l)+O2(g) You may want to reference (Page) Section 6.1 while completing this problem. Part A How many milliliters of O2(g)O2(g) at 27 ∘C∘C and 5.00 barrbarr can be liberated from 18.95 mLmL of an aqueous solution containing 3.00%% H2O2H2O2 by mass? The density of the aqueous solution of H2O2H2O2 is 1.01g/mLg/mL.

Calculate the equilibrium constant for each of the reactions at 25 ∘C. Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq) Express...

Calculate the equilibrium constant for each of the reactions at 25 ∘C. Part B O2(g)+2H2O(l)+2Cu(s)→4OH−(aq)+2Cu2+(aq) Express your answer using two significant figures.

1)Given the following data: 2H2(g) + O2(g) → 2H2O(l) ΔH = -571.6 kJ CO2(g) + 2H2O(l)...

1)Given the following data: 2H2(g) + O2(g) → 2H2O(l) ΔH = -571.6 kJ CO2(g) + 2H2O(l) → CH4(g) + 2O2(g) ΔH = +890.3 kJ C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ Find the ΔH of the following reaction: C(s) + 2H2(g) → CH4(g)

Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g)  2H2O(l) + 2 Cl2(g)...

Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g)  2H2O(l) + 2 Cl2(g) ΔHrxn = + 96.976 kJ/mol B.If you place 750 mL of 0.500 M solution of HCl with 17.2 g of O2, will any oxygen remain? (Hint: limiting reagent problem) C.What mass of chlorine gas (in grams) is produced? D) How many molecules of Cl2 are produced based on part (B) E) What mass of excess reagent remains after the limiting reagent is used up?...

Preparation of CuCl Reactions: 1) Cu(S) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) 2) 2HNO3(aq)...

Preparation of CuCl Reactions: 1) Cu(S) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) 2) 2HNO3(aq) + Na2CO3(s) -> H2O(l) + CO2(g) + 2NaNO3(aq) 3)Cu(NO3)2(aq) + Na2CO3(s) -> CuCO3(s) + 2NANO3(aq) 4)CuCO3(s) + 2HCL(aq) -> CuCl2(aq) + H2O(l) + CO2(g) 5)CuCl2(aq) + Cu(s) -> 2CuCl(s) Weight of copper: 1.023g Volume of Added Nitric Acid: 5.5 mL Total weight of added Sodium Carbonate: 3.85g Weight of Watch Glass and filter paper: 51.533g Weight of Watch Glass, Filter Paper and CuCl Precipitate:...

Classify the following chemical reactions:  _H2SO4(aq) + 2KOH(aq) →2H2O(l) + K2SO4(aq) _3Mg(s) + N2(g) —> Mg3N2(s)...

Classify the following chemical reactions:  ___H2SO4(aq) + 2KOH(aq) →2H2O(l) + K2SO4(aq) ___3Mg(s) + N2(g) —> Mg3N2(s) ___H2CO3(aq) —> CO2(g) + H2O(l) ___C3H8(s) + 5O2(g) —> 3CO2(g) + 4H2O(g) a. precipitation b. redox c. combustion d. neutralization e. gas evolution

Hess's Law Calculate the Value of H for: 3NO2(g)+2H2O(l) = 2HNO3(aq)+NO(g) Using this information: 2NO(g)+O2(g) =...

Hess's Law Calculate the Value of H for: 3NO2(g)+2H2O(l) = 2HNO3(aq)+NO(g) Using this information: 2NO(g)+O2(g) = 2NO2(g) , H=-116 kJ 2N2(g)+5 O2(g)+2H2O(l) = 4HNO3(aq) , H= -256kJ N2(g) + O2(g) = 2NO(g) , H=+183kJ

Question