H2O2(aq) --> H2O(l) + O2(g) 1. identify half rxns and overall balanced equation. 2. what is E° of the cell? 3. [H2O2]...
H2O2(aq) --> H2O(l) + O2(g)
1. identify half rxns and overall balanced equation.
2. what is E° of the cell?
3. [H2O2] = 0.2 M, Po=0.21 atm, other species still have concentration of 1.0 M. What is cell potential?
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H2O2(aq) --> H2O(l) + O2(g) 1. identify half rxns and overall balanced equation. 2. what is E° of the cell? 3. [H2O2]...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½ O2(g)...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq)H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3 min-1. If the initial concentration of H2O2 is 5.66×10-2 M, the concentration of H2O2 will be 9.34×10-3 M after _______ min have passed.
In the chemical equation H2O2(aq) → H2O() + O2(g), the O2 is a _ O reactant...
In the chemical equation H2O2(aq) → H2O() + O2(g), the O2 is a _ O reactant O product catalyst inhibitor solid
H2O2(aq)⟶H2O(l) + 1/2 O2(g) a. The above chemical equation is for a first-order reaction. At 302...
H2O2(aq)⟶H2O(l) + 1/2 O2(g) a. The above chemical equation is for a first-order reaction. At 302 K , the rate constant equals 8.5×10−4s−1. Calculate the half-life at this temperature. Express your answer to two significant figures and include the appropriate units. b. If the activation energy for this reaction is 75 kJ/mol, at what temperature would the reaction rate be doubled? Express your answer as an integer and include the appropriate units.
2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solutio...
2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solution of H2O, that is 6.00 percent H,O, by mass has a density of 1.03 g ml. Calculate each of the following. (i) The original number of moles of H2O, in a 125 ml sample of the 6.00 percent H2O2 solution (ii) The number of moles of O,(g) that are produced when all of the H2O2 in the 125 mL sample...
1) The enthalpy of formation for H2O(l) is given by H2(g) + 1/2 O2(g) → H2O(l)....
1) The enthalpy of formation for H2O(l) is given by H2(g) + 1/2 O2(g) → H2O(l). Add this reaction to H2O(l) + 1/2 O2(g) → H2O2(aq). This is the reverse of the decomposition reaction from this experiment. Show the sum of the above two reactions is the enthalpy of formation of H2O2(aq) 2) Calculate the literature value for the enthalpy of decomposition of H2O2(aq) from the enthalpies of formation of H2O2(aq), H2O(l) and O2(g) found in your textbook or any...
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) +...
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) + 1/2 O2(g) 26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(2) + 1/2O2(g) At 20.0 °C, the half-life for the reaction is 3.05 x 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 8.00 days?
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order...
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq) ------> H2O(l) +...
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H2O2(aq) ------> H2O(l) + ½ O2(g) is first order in H2O2 with a rate constant of 1.10×10-3min-1. If the initial concentration of H2O2 is 5.52×10-2 M, the concentration of H2O2 will be 1.56×10-2 M after _____ min have passed.
Enter the balanced complete ionic equation for HCl(aq)+K2CO3(aq)→H2O(l)+CO2(g)+KCl(aq). Express your answer as a chemical equation. Identify...
Enter the balanced complete ionic equation for HCl(aq)+K2CO3(aq)→H2O(l)+CO2(g)+KCl(aq). Express your answer as a chemical equation. Identify all of the phases in your answer.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential O2...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential O2 (g) + 4H+ (aq) +4e− → 2H2O (l) =E0red+1.23V Zn+2 (aq) +2e− → Zn (s) =E0red−0.763V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is...
In the chemical equation H2O2(aq) → H2O() + O2(g), the O2 is a _ O reactant O product catalyst inhibitor solid
2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solution of H2O, that is 6.00 percent H,O, by mass has a density of 1.03 g ml. Calculate each of the following. (i) The original number of moles of H2O, in a 125 ml sample of the 6.00 percent H2O2 solution (ii) The number of moles of O,(g) that are produced when all of the H2O2 in the 125 mL sample...
26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(l) + 1/2 O2(g) 26. Hydrogen peroxide decomposes into water and oxygen in a first-order process. H2O2(aq) → H2O(2) + 1/2O2(g) At 20.0 °C, the half-life for the reaction is 3.05 x 104 seconds. If the initial concentration of hydrogen peroxide is 0.52 M, what is the concentration after 8.00 days?
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