Ans-
Available chlorine is calculated as if Cl2 was present as the oxidizing agent. This can be done, because both Cl2 and ClO- react with the iodide ion, I-, in a 1:1 stoichiometry as shown in the equations below.
Cl2(g) + 2 I-(aq)® 2 Cl-(aq) + I2(aq)
ClO-(aq) + 2 I-(aq) + H2O(l) ® I2(aq) + Cl-(aq) + 2 OH-(aq)
Available chlorine is reported as the mass of chlorine per unit mass of solution, or powder if this is a dry chlorine bleach. This mass ratio is frequently converted to a percent and reported as the percent available chlorine.
Chlorine is soluble in water and its dissolution in water is a physical and chemical process. 2, 4 Upon contact with water, chlorine disproportionates , giving chloride ion and hypochlorous acid 2, 8 or hypochlorite ion, depending on the pH of the solution. Thus, dissolved chlorine is present in aqueou 2 s solutions as a mixture of three active species, molecular chlorine (Cl ), hypochlorous acid (HOCl), and hypochlorite ion (OCl ). These three species are generally called free available chlorine – 9 (FAC). The distribution of these species can be described by the following equations 8 Cl2 2 H + H O ¾ Cl + H + HOCl K = 4×10 (25°C)
–4 HOC a l ¾ H + OCl pK = 7.54 (25°C) (2) + –
Both equilibria are pH dependent. Thus, the distribution of the three species varies with the pH of the solutions. By using the equilibrium constants,
Calculate the percent available chlorine in chlorine dioxide (C102).
: Chlorine dioxide (C102) has been tested as a disinfectant for water treatment and is produced by the following reaction 2NaClO2(aq) + Cl2(g) → 2C102(g) + 2NaCl(aq) a) Calculate Eº, AGº and K at 25°C for the production of ClO2 using appropriate data. b) A major concern for using C1O2 as a disinfectant is that a possible by-product, the chlorate ion (CIO3-) could be produced as follows ClO2(g) = C103-(aq) + Cl-(aq) Balance the above equation.
In one experiment, 17.8 g of chlorine were used and yielded 43.5 g of chlorine dioxide- CIO2. b. Calculate i) the theoretical yield (in grams) of chlorine dioxide- CIO2 ii) The % yield of chlorine dioxide
In one experiment, 17.8 g of chlorine were used and yielded 43.5 g of chlorine dioxide- CIO2 b. Calculate i) the theoretical yield (in grams) of chlorine dioxide- CIO2 The % yield of chlorine dioxide ii)
Calculate ΔG° in kJ at 15.4 °C for the reaction of sulfur dioxide gas with chlorine gas to form sulfur oxydichloride gas and chlorine oxide gas. Be sure to balance the reaction using the lowest whole numbers. Use ΔH° and ΔS° to calculate and assume that they are independent of temperature. Use the thermodynamic data provided in the Extras folder on BlackBoard. Report your answer to one place past the decimal.
Chlorine dioxide (ClO2) is produced by the following reaction: 2 NaClO2(aq) + Cl2(g) ® 2 ClO2(g) + 2 NaCl(aq) Calculate E°, ΔG°, and K at 25 °C for the production of ClO2. Note: Na+ is a spectator ion. ClO2 + e- → ClO2- Ɛ° = 0.954 v
Calculate (H+), [C102], and (OH) in an aqueous solution that is 0.165 M in HCIO, (aq) at 25 °C. [c107] = [OH-] = 1 Is the solution acidic, basic or neutral? acidic O basic O neutral
Determine the oxidation potential for converting chloride (Cl-) to chlorate (ClO3-) from a). the chlorine dioxide/chloride reaction b). the chlorine dioxide/chlorite reaction c). the chlorate/chloride reaction
5. Calculate the percent copper and percent chlorine for the following compound: Cu2Cl Group of answer choices 50.00% Cu, 50.00% Cl 28.55% Cu, 71.45% Cl 71.45% Cu, 28.55% Cu 78.19% Cu, 21.81% Cl 21.81% Cu, 78.19% Cl 6. Calculate the percent copper and percent chlorine for the following compound: CuCl2 Group of answer choices 78.19% Cu, 21.81% Cl 21.81% Cu, 78.19% Cl 47.26% Cu, 52.74% Cl 52.74% Cu, 47.26% Cl 25% Cu, 75% Cl 7. Using the following data and...
If the percent chlorine in a salt crystal, KCl is 47.55 %, what is the percent chlorine in a kilogram of salt?
Chlorine and oxygen gases react to form chlorine dioxide gas. Cl2(g) + 2 O2(g) 2 ClO2(g) At a certain temperature and pressure 1.4 L of Cl2 reacts with 2.8 L of O2. If all the Cl2 and O2 are consumed, what volume of ClO2, at the same temperature and pressure, will be produced? L