Q: In a certain zinc-copper cell, Zn(s) + Cu2*(aq) –→ Zn²*(aq) + Cu(s) the ion concentrations are…
A: Given equation : Zn(s) + Cu2+ (aq) -------> Zn2+ + Cu(s) [Cu2+] = 0.0195M [Zn2+] = 1.4M Ecell =…
Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…
A: In electrochemical cell , the value of potential difference between two electrodes is known as cell…
Q: The cell potential for this reaction is V when the concentration of [Cu2*] = 1.0 x 105 M and [Zn2*]=…
A:
Q: In a certain zinc-copper cell, Zn(s) + Cu2+(aq) – Zn2*(aq) + Cu(s) the ion concentrations are [Cu2*]…
A: Given reaction is : Zn (s) + Cu2+ (aq) --------> Zn2+ (aq) + Cu (s) [Cu2+] = 0.0234 M [Zn2+] =…
Q: two identical pieces of the same unknown metal are placed into 1.0 M solutions of aqueous LiNO3 and…
A:
Q: 1. Based on the standard reduction potentials in Table 2, which of the following metals could…
A: The metals given are Al, Cu, Ni and Zn.
Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.825 M and…
A: Answer = 0.464 V
Q: Calculate the cell potential for the reaction as written at 25.00 °C , given that [Mg2+]=0.874 M and…
A: According to the Nernst equation, the cell potential is given by Ecell = E0cell - (0.0591/n) log(Q)…
Q: In a certain zinc-copper cell, Zn(s) + Cu2*(aq) –→ Zn?*(aq) + Cu(s) the ion concentrations are…
A:
Q: Use the Nernst equation to calculate the cell potential for the following cell in Volts: Cr|Cr3+,…
A: The cell given is, => Cr (s) | Cr3+ (aq, 0.0010 M) || Cu2+ (aq, 1.0 M) | Cu (s)
Q: Calculate the cell potential for the following reactions and predict whether the reaction will take…
A: The given redox reaction is as follows: Zn(s) + 2Ag+(aq) → Zn2+ + 2Ag Two half cell reactions and…
Q: 18.39 Consider the following galvanic cells: 1. Cu(s)|Cu²*(1 M) || Fe³*(1 M), Fe²*(1 M)|Pt(s)
A: The balanced chemical reaction is the one that contains equal number of atoms on both sides of the…
Q: If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0M, what is the…
A: Given, The cell emf of a Zn-Cu cell is 0.80 V.The concentration of Cu2+when the concentration of…
Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…
A: We have tp Calculate the standards potential value for the following cell reaction…
Q: The free energy change for the following reaction at 25 °C, when [Zn²+] = 4.75×10³ M and [Ni2*] =…
A: Answer: These questions are based on relationship between Gibbs free energy change and cell…
Q: Write the cell notation. Fe- | Fe || Cu | Cu2+ B Fe | Fe2* || Cu* | Cu (© Cu" | Cu || Fe Fe Fe2 Fe
A: Cell notation We first write the anode half cell salt bridge then cathode half cell Always remember,…
Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that (Zn+) = 0.773 M and…
A:
Q: Consider a battery with the overall reaction: Cu(s) + 2Ag+(aq) ⟶ 2Ag(s) + Cu2+(aq).A battery is…
A: Using Nernst equation we can write that, When battery is dead then the ratio of…
Q: In a certain zinc-copper cell, Zn(s) + Cu²*(aq) –→ Zn2*(aq) + Cu(s) the ion concentrations are…
A: Given reaction is : Zn (s) + Cu2+ (aq) -> Zn2+ (aq) + Cu (s) [Cu2+] = 0.0397 M [Zn2+] = 1.8 M…
Q: Which of these metals does not act as a sacrificial electrode for iron?Zn, Mg, Mn, Cu
A: The standard electrode potentials of given metals are Mg: -2.36 V Zn: -0.76 V Mn: -1.185 V Cu: +0.34…
Q: Write a balanced chemical equation for the overall cell reaction represented as a) Fe"/Fe* //…
A:
Q: If the concentration of Cd2+ is reduced to 0.010 M, and [Ni2+] = 1.0 M, what is the new cell…
A:
Q: n electrochemical cell has an iron electrode in a solution of Fe2+ ions on one side, and a nickel…
A: Electrochemical series is an activity series that tells the arrangement of elements in order of…
Q: A concentration cell contains Cu2+ ions in solution in both ½ cells. If the electrons flow from left…
A: The concentration cell is made by using the solution of same electrolyte in different concentrations…
Q: a. Calculate the equilibrium constant for the following reaction at 25°C: Ag* (aq) + Fe2+ (ag) →…
A:
Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2 +] = 0.887 M…
A:
Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and…
A: Cr(s)+Fe+2 (aq )<==> Cr+2 (aq)+Fe(s) [Cr+2] = 0.876 M [Fe+2] = 0.0120 M
Q: Calculate the cell potential for the following concentration cell at 25 °C.…
A: Here the cell represented consists of a cathode and the anode made up of nickel. In the cell…
Q: In a certain zinc–copper cell, Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) the ion concentrations are [Cu2+]…
A:
Q: A copper-silver cell is set up. The copper ion concentration is 0.10 M. The concentration of silver…
A: Given : Cell potential, Ecell = 0.422 V Concentration of Copper ion, [Cu2+ ] = 0.10 M Standard…
Q: Which would the cell potential be if you changed the concentrations to [Fe3*] = 0.60 [Hg²*) = 1.30 M…
A: The Nernst equation is shown below: Where: Ecell = cell potential E0cell = standard cell potential…
Q: What is the Eocell value for the reaction represented by the following cell diagram? Pt(s) | O2(g)…
A: Given : Pt(s) | O2(g) | H2O2(aq) || Cu2+(aq) | Cu(s)
Q: 19.85 Calculate the cell potential of the following cell at 25°C. Cr(s) Cr **(1.0 x 10 ³ M) | |…
A:
Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…
A: Standard reduction potential of nickel = -0.257 V Standard reduction potential of silver = 0.7996 V…
Q: Use the standard cell potential to calculate the value of the equilibrium constant, K, at 25°C for…
A: The electrochemical cell that utilized energy released from spontaneous chemical reaction to produce…
Q: A concentration cell is constructed by placing identical Cu electrodes in two Cu2+ solutions. If the…
A: E◦ for Cu2+ to Cu is 0.342. But concentration cell is formed with same metal. So the E◦cell is 0.
Q: In a certain zinc-copper cell, Zn(s) + Cu2*(aq) → Zn2*(aq) + Cu(s) the ion concentrations are [Cu2+]…
A: Goven Zinc-Copper cell is Zn(s) + Cu2+(aq) ---> Zn2+(aq) + Cu(s) Concentration of Cu2+ , [Cu2+]…
Q: Write the cell diagram for the following cell. + V KCI(aq) Hg,Cl2(s) Pt Hg(1) ZnCl2(aq) uz
A: Anode reaction - Hg(l) ------> Hg2+(aq) + 2e Cathode reaction - Zn2+(aq) + 2e -----> Zn(s)…
Q: For the cell Cr | Cr3+ || Co2+ | Co E o is 0.46V. The same cell was prepared in the laboratory at…
A: The standard reduction potential of chromium is -0.74 V and the standard reduction potential of…
Q: A copper-silver cell is set up. The copper ion concentration is 0.10 M. The concentration of silver…
A: Given [Cu2+] = 0.10 M Ecell = 0.422 V E0Ag+/Ag= +0.80 E0Cu2+/Cu = +0.34 V Cu + 2Ag+(aq) →…
Q: Calculate the cell potential for the following concentration cell at 25 °C.…
A: Given Concentration cell Ni(s)|Ni(NO3)2(0.00522 M)|| Ni(NO3)2(3.07 M)| Ni(s) Ni…
Q: How many seconds does it take to deposit 84.6 g of Zn on a steel gate when 21.0 A is passed through…
A: According to Faraday first law chemical deposition of element is directly proportional to quantity…
Q: In a certain zinc-copper cell, Zn(s) + Cu2+(aq) –→ Zn²+(aq) + Cu(s) the ion concentrations are…
A:
Q: Calculate the cell potential of the following cell at 25°C. Cr(s)|Cr³*(1.0 × 10-3 M)||Ni²*(1.5…
A: The half-cell reaction involved in the given cell and the standard reduction potential is given…
Q: Consider the cell diagram: Sn|Sn+2 (aq)||NO(g)|NO3-(aq)|Pt(s) Identify the reducing agent (A)NO…
A: The given cell notation is,
Q: Write the cell notation for an electrochemical cell consisting of an anode where Mn (s) pxidized to…
A: Anode : Mn(s) → Mn2+(aq) + 2e- Cathode : Cr3+(aq) + 3e- → Cr(s)
Q: For the cell diagram: Mg(s)|Mg2+(aq)|2H+(aq)|H2(g)|Pt(s) which reaction occurs at the anode?
A:
Q: If the cell emf of a Zn-Cu cell is 0.80 V when the concentration of Zn2+ is 2.0 M, what is the…
A: The emf of Zn-Cu cell = 0.80 V Concentration of Zn2+ = 2.0 M Concentration of Cu2+ (in molar) = ?
rearrange the reaction to make it spontaneous then write the cell diagram
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- What is the difference between iron and steel? What is the difference between wrought iron and cast iron?Which of the following is a transition metal? a) Aluminum b) Copper c) Zinc d) SodiumSterling silver (silver 925) is a substitutional solid solution alloy consisting of 92.5 wt% Ag and 7.5 wt% Cu. Compute the number of Cu atoms per cubic centimeter of silver 925. The density of the pure Ag and Cu are 10.49 g/cm3 and 8.96 g/cm3, respectively.
- Cu(s) + NO3-(aq) → Cu2+(aq) + NO2(g) Referring to the equation above, what is the oxidation number of Cu in Cu(s)?How to write a chemical equation for transition metal ions found in a solution? The ions found were Cobalt and Copper. Co2+ (aq) + Cu2+ (aq) was mixed with NaOH (aq). It formed Co(OH)2 (s) + Cu(OH)2 (s) + Na^+ (aq). The sample was decanted and Na+ was removed. NH3(aq) was added to Co(OH)2 (s) + Cu(OH)2 (s) and became Co(OH)2 + Cu(NH3)4 ^2+ and NH3. The sample was centrifuged and decanted the ions were now in their own tubes. One tube had Co(OH)2 and the other had Cu(NH3)4 ^2+ and NH3. The tube with Co(OH)2 was then mixed with HNO3 and became Co^2+. The tube with Cu(NH3)4 ^2+ and NH3 was mixed with HNO3 and became Cu^ 2+ and NH4^+.FeO + Zn(s) --------->. ZnO + Fe(s)What is the Oxidizing Agent?
- In the compound Pt(C2H3O2)2, what is the charge on the platinum?A prospector wants to know how much gold is in the ore that he has been mining. A sample weighing 11.2456 grams is dissolved in Aqua Regia (a mixture of HCl and HNO3). That sample is then transferred to a 200.00 mL volumetric flask and diluted to the mark with water. This is called solution 1. A volumetric pipet is used to transfer 10.00 mL of solution 1 to a second 500.00 mL volumetric flask. The second flask is filled to the mark resulting in solution 2. 5.00 mL of solution 2 is analyzed and found to contain 13.45 ppm Au. Answer each of the questions below. 1. What is the concentration of Au in solution 1. The units should be ppm 2. How many micrograms of Au are in the 5.00 mL sample that was measured? 3. How many micrograms of gold were in the 500.00 mL flask containing solution 2. 4. How many grams Au were in the flask containing solution 1 5. What is the %Au in the original sample?Chemistry The initial abundances of O, Mg, and Si atoms are respectively in the ratio 21:1:1.And O, Mg, and Si respectively have atomic masses of 16, 24, and 28 a.m.u. Assuming a planet is made of olivine minerals (Mg2SiO4), how many O atoms are left over for every 2 Mg atoms used? Assuming the extra O atoms combine with hydrogen to form H2O, what is the mass ratio of water to rock in this planet?
