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Given the following reaction in acidic media:
Fe2+ + Cr2O72- --> Fe3+ + Cr3+
The coefficient for water in the balanced reaction is _________.
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- A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.Given the following reaction in acidic media: Fe2+ + Cr2O72- ® Fe3+ + Cr3+answer the following question: The coefficient for water in the balanced reaction is:Zinc(s) (MW=65.38), with a mass of 0.825 g, was reacted with 25.00 mL of NaClO (MW=74.44) according to the following unbalanced ionic equation. Determine the normality of NaClO.Zn(s) + ClO- → Zn(OH)2 + Cl- (in basic medium)
- Which of the following is wrong for erosive corrosion? A: Occurs when corrosive solutions flow rapidly from the metal surface B: The main effect of erosion is that corrosion products are dragged away by the fluidC: If the liquid carries solid particles or if there are air bubbles, the severity of erosion corrosion increases D: Metals with passivation feature do not undergo erosive corrosion E: The metals most susceptible to erosive corrosion are copper and copper alloysA piece of an unknown weighing 12.50is placed in 49.7cm of water in a cylinder. The water level increases to 69.0cm3. whats the calculated value for the drnsity of the solid in g ml-1Black-and-white photographic film is coated with silver halides. Because silver is expensive, the manufacturer monitors the Ag⁺ content of the waste stream, [Ag⁺]ᵥᵥₐₛₜₑ, from the plantwith an Ag-selective electrode at 25°C. A stream of known Ag⁺ concentration, [Ag⁺](standard), is passed over the electrode inturn with the waste stream and the data recorded by a computer.(a) Write the equations relating the nonstandard cell potential tothe standard cell potential and [Ag⁺] for each solution.(b) Combine these into a single equation to find [Ag⁺]ᵥᵥₐₛₜₑ.(c) Rewrite the equation from part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ in ng/L.(d) If Eᵥᵥₐₛₜₑ is 0.003 V higher than E(standard), and the standard so-lution contains 1000. ng/L, what is [Ag⁺]ᵥᵥₐₛₜₑ?(e) Rewrite the equation in part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ for a sys-tem in which T changes and Tᵥᵥₐₛₜₑ and T(standard) may be different.
- In an experiment to check chemical balance, measurements of electrical conductivity (κ) were made of acid solutions in different concentrations, as shown in the table below. From these data, show that the acetic acid dissociation equilibrium constant is really a constant, that is, it has the same value for any acetic acid solution at a given temperature. The data were collected at 25 oC. The limit molar conductance of the acetic acid solution is Λ0 = 390.71 Ω^-1*cm^2 / mol. Suggestion: calculate the molar conductance (Λm = 1000 κ / c) for each concentration and then use Ostwald's Dilution Law Molarity c (mol / L) Conductivity κ (Ω^-1*cm^-1) 0.010 1.5590 x 10^-4 0.05 3.5939 x 10^-4 0.1 5.0610 x 10^-4 ANSWER: values close to 1.7 x 10^-5 I need the calculations to show how to obtain this valueThe iodine produced when excess of KI was added to the solution containing 0.1259 g K2Cr2O7 required a 41.26 mL titration with Na2S2O3 required a 41.26 mL titration with Na2S2O3. P.S. Be able to answer numbers 1 and 2 ONLY. 1. Determine if it is basic or acidic and write the balance redox reaction for the reaction of dichromate ion with iodide ion in acidic medium. Unbalance equation: Cr2O72- (aq) + I- (aq) → Cr3+ + I2 (aq) 2. Determine if it is basic or acidic and write the balance redox reaction of iodine with sodium thiosulfate in acidic medium. Unbalance equation: S2O3 2- (aq) + I2 (aq) → S4O6 2- (aq) + I- (aq) 3. (i) What are the oxidizing agents in #1 and #2? (ii) What is the stoichiometric ratio between dichromate and thiosulfate? 4. Calculate the molar concentration of the thiosulfate solution.1.How many grams of NaCl is present on 5.0 mL of 1.0 % m/V NaCl solution? 2. A zinc bar weighing 3.0 kg is attached to a buried iron pipe to protect the pipe from corrosion. An average current of 0.020 A flows between the bar and the pipe. How many years will be required for the zinc bar to be entirely consumed?
- The solubility-product constant for Ag2SO3 is 1.5x10-14. Calculate E0 for the processConsider the Gibbs energies at 25 ∘25 ∘C. SubstanceSubstance Δ?∘f (kJ·mol−1)ΔGf∘ (kJ·mol−1) Ag+(aq) 77.1 Cl−(aq) −131.2 AgCl(s) −109.8 Br−(aq) −104.0 AgBr(s) −96.9 (a) Calculate Δ?∘rxn for the dissolution of AgCl(s). (b) Calculate the solubility-product constant of AgCl. (c) Calculate Δ?∘rxn for the dissolution of AgBr(s). (d) Calculate the solubility-product constant of AgBr.Zinc(s) (MW=65.38), with a mass of 0.228 g, was reacted with 20.00 mL of NaClO (MW=74.44) according to the following unbalanced ionic equation. Determine the normality of NaClO. Zn(s) + ClO- → Zn(OH)2 + Cl- (in basic medium)
