The overall reaction of a mercury cell is
Zn(s) + HgO(s) + H2O(l) → Zn(OH)2(s) + Hg(l)
If a mercury cell contains 0.100 g of HgO, and the HgO is the limiting reagent, the time (days) for which a current of 1.00 × 10-5 A could flow from the cell is
D. 51.2
The overall reaction of a mercury cell is Zn(s) + HgO(s) + H2O(l) → Zn(OH)2(s) +...
Mercury cells as “button” batteries are very common and consist of HgO, ZnO, and Zn(OH)2 in a KOH paste. Useful half-cell reactions: HgO(s) + H2O(l) + 2e = Hg(l) + 2OH-(aq) eo = 0.0977 V Zn(OH)42-(aq) + 2e = Zn(s) + 4OH-(aq) eo = -1.285 V Zn(OH)42-(aq) = ZnO(s) + H2O(l) + 2OH-(aq) A)Such batteries have a + sign marked on them. Which half-reaction is occurring at the electrode so marked? B)Draw a schematic of a mercury...
In the reaction, 2 HgO(s) → 2 Hg(s) + 0,() what mass of mercury(II) oxide, HgO, would be required to produce 519 L of oxygen, O, measured at STP? mass: A student needs to prepare 50.0 mL of a 0.80 M aqueous H, O, solution. Calculate the volume of 4.9 MH,O, stock solution that should be used to prepare the solution. volume: ml How many grams of sodium hydroxide are present in 247.0 mL of a 0.300 M NaOH solution?...
You are given the following reduction half reactions in basic solution: 2 NO2-(aq) + 3 H2O(l) + 4 e- →N2O(g) + 6 OH-(aq) E° = 0.1500 V HgO(s) + H2O(l) + 2 e- → Hg(s) + 2 OH-(aq) E° = +0.0984 V A. If this redox reaction occurs, how many total electrons will have to be transferred per mole of reaction? N2O(g) + 2 OH-(aq) + 2 HgO(s) → 2 NO2-(aq) + H2O(l) + 2 Hg(s) B. What is the...
described in (a). 11. Joseph Priestley's study of the decomposition of mercury(II) oxide (HgO) with heat led to the discovery of O2. The balanced equation for this reaction is shown in Equation 9. (Eq. 9) beat 2 HgO(s) 2 Hg()+O2(g) (a) How many grams of O2 could possibly be formed by the decomposition of 75.0 g of HgO? (b) How many grams of HgO must be decomposed to produce 75.0 g of O2? 12. Propane (CHs) is used as a...
Table 1 Cell Type Lithium-iodine Zinc-mercury Operating Cell Potential for Commercial Batteries, E (V) +2.80 +1.35 Table 2 Standard Reduction Potential, E" (V) Half-Reaction Zn(OH).1? +2e → Zn +40H Zn(OH), +2e → Zn +20H HgO + H2O +2e - Hg + 2OH 0, + 2 H2O + 4e 40H - 1.20 |--1.25 +0.10 +0.40 Pacemakers are electronic devices that help regulate the heart rate. Currently, lithium-iodine cells are commonly used to power pacemakers and have replaced zinc-mercury cells. Table 1...
A digital watch battery draws 0.25 milliamperes of current, which is provided by a mercury battery whose net reaction is: HgO(s) + Zn(s) → ZnO(s) + Hg(l) If a partially used battery contains 0.50 g of each of these four substances, for how many hours will the watch continue to run?
A digital watch battery draws 0.25 milliamperes of current, which is provided by a mercury battery whose net reaction is: HgO(s) + Zn(s) → ZnO(s) + Hg(l) If a partially used battery contains 0.50 g of each of these four substances, for how many hours will the watch continue to run?
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Ats In the reaction, 2 HgO(s) 2 Hg(s) + O2(g) what mass of mercury(II)oxide, HgO, would be required to produce 935 L of oxygen, O, measured at STP? mass: about us career privacy policy terms of use contact us
Consider an electrochemical cell based on the following reaction: Zn(s) + 2H2O(l) + 2OH-(aq) ⇄ [Zn(OH)4]2-(aq) + H2(g) All dissolved species are at 2.5 x 10-3 M; pressure of H2 is 1 bar (standard state) Use the Nernst equation to calculate E.
Consider the reaction below Al2S3(s) + H2O(l) → Al(OH)3(s) + H2S(g) If 15.0g of aluminum sulfide and 10.0g of water are allowed to react as above, and assuming a complete reaction a. by calculation, find out which is the limiting reagent. b. calculate the maximum mass of H2S which can be formed from these reagents. c. calculate the mass of excess reagent remaining after the reaction is complete.