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The overall reaction for the discharge of a nonrechargeable alkaline battery is 2MnO2(s) + Zn(s) +...
) The discharge reaction for a zinc-manganese dioxide battery can be represented as: Zn(s) + 2MnO2(s) → ZnO(s) + 2Mn2O3(s) What quantity of charge (in coulombs) can be provided by a fully charged 1.50-V zinc-manganese dioxide photo-flash battery, if the mass of MnO2 in the battery is 9.90 g? C (b) What is the maximum amount of work (in joules) that can be obtained from this battery? J
The discharge reaction for a zinc-manganese dioxide battery can be represented as: Zn(s) + 2MnO2(s) → ZnO(s) + 2Mn2O3(s) (a) What quantity of charge (in coulombs) can be provided by a fully charged 1.50-V zinc-manganese dioxide photo-flash battery, if the mass of MnO2 in the battery is 8.83 g? C (b) What is the maximum amount of work (in joules) that can be obtained from this battery? J
Whats the oxidizing agent in this reaction? Zn+ 2MnO2+2H2O -> Zn(OH)2 +2MnO(OH)
During the discharge (operation) of a 1.5 alkaline battery, Robin determined that 6.33g of zinc was oxidized to zn(oh)2. a) what mass of Mno2 was reduced at the cathode. b) How many coloumbs of electron charge we're transferred from zn to Mno2 ? c) How many joules of electrical energy we're produced ?
If a 1.5 V AAA alkaline battery can power a 1.4 Watt device for 1 hour, how many grams of zinc (65.38g/mol) does it contain? Overall reaction in battery: MnO2 + 2H2O + Zn --> Mn(OH)2+ ZnO The answer is 1.1 g Please explain step by step and how to reach this answer.
During the discharge of an alkaline battery, 4.10 g of Znare consumed at the anode of the battery. A. What mass of MnO2 is reduced at the cathode during this discharge? B. How many coulombs of electrical charge are transferred from Zn to MnO2? Please explain this question to me.
using Hess's law what is the standard enthalpy of formation of manganese(ll)oxide, MnO(s)? 2MnO2(s)-->2MnO(s)+O2(g) rxn= +272.0 kJ/mol MnO2(s)+Mn(s)-->2MnO(s) rxn=-248.9 kJ/mol A. -520.9 kJ/mol B. -396.5 kJ/mol C. -384.9 kJ/mol D. -147.6 kJ/mol E. 24 kJ/mol
In kJ If an alkaline battery produces a cell potential of 1.62 V, what is the value of AG cell? The half-reactions in alkaline batteries are: Zno(s) +H,0(1) +2e → Zn(s) +20H (aq) 2MnO2 (s) +H20(1) +22 → Mn,oz (s) +20H (aq)
3. A typical construction of the most commonly used alkaline battery (AA, AAA etc) is shown as follows: POSITIVE CONNECTION (stainless steel electrode) CURRENT PICK UP ZINC ANODE (2n powder in aqueous KOH paste) ION CONDUCTING SEPARATOR (Porous cellulose or polyethylene film saturated with aqueous KOH) MANGANESE OXIDE CATHODE (MnO+graphite powder in aqueous KOH paste) OUTER CASING PRESSURE EXPANSION SEAL PROTECTIVE CAP NEGATIVE TERMINAL (stainless steel electrode) Anode Zn (s)+20H (aq) -2e ZnO (s)+H2O D, Cathode: 2MnO2 (s+HOMn O (s)...
07 Question (1 point) If an alkaline battery produces a cell potential of 1.48 V, what is the value of God? The half-reactions in alkaline batteries are: ZnO(s) +H,0(1) +20 - Zn(s) - 20H(aq) 2MnO, (s) +H,0() +20" Mn,0, (s) +20H(aq) 5th attempt See Periodic Table See Hint Feedback AG 2.36