11.4. The reactions of chlorine
A subsection of Chemistry, 9701, through 11. Group 17
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Chlorine is a very reactive element. Chlorine reacts with silicon to form silicon(chloride. Describe the appearance of silicon(chloride at room temperature and pressure. State its structure and bonding. appearance structure and bonding Samples of magnesium chloride and phosphorus(chloride are added to separate beakers of cold water. Complete Table 3.1. Ignore temperature changes when considering observations for these reactions. Table 3.1 magnesium chloride phosphorus(chloride appearance at room temperature one similarity in observation on addition to cold water one difference in observation on addition to cold water pH of final solution State the reagent and conditions required for the formation of sodium chlorate(from Cl 2. Explain why the reaction in is described as a disproportionation reaction. Your answer should refer to relevant species and their oxidation numbers. Chlorine reacts with methane in a series of reactions to produce chloroalkanes. State the conditions required for chlorine to react with methane. One of the products of the reaction is CH2Cl 2 which reacts further to produce CHCl 3. Complete Table 3.2 to show details of the mechanism that forms CHCl 3 from CH2Cl 2. Table 3.2 name of step equation initiation propagation CH2Cl 2 + Cl • termination CHCl 3 CHCl 3 and HF are used to form CHCl F2 in a substitution reaction. Construct an equation for this reaction. X is a product of the substitution reaction that occurs when CHCl F2 reacts with Br2. There is only one naturally occurring isotope of fluorine, 19F. The mass spectrum of X shows molecular ion peaks at m / e = 164, 166 and 168. Complete Table 3.3 to show all the molecular ions responsible for each peak. Table 3.3 m / e formulae of molecular ions (CF2 37Cl 81Br)+
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THEORY
2023
Paper 2, Variant 1
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Chlorine is a reactive element. It forms many compounds. Complete Table 2.1 to show the maximum oxidation number of the elements Na to P in their chlorides. Table 2.1 element Na Mg Al Si P maximum oxidation number State what determines the maximum oxidation number of elements in Period 3. An excess of cold water is added to the chloride of silicon. Write an equation for the reaction between an excess of cold water and the chloride of silicon. Suggest the pH of the solution produced in . An excess of cold water is added to the chloride of phosphorus. Write an equation for the reaction between an excess of cold water and the chloride of phosphorus. Suggest the pH of the solution produced in . Write an equation for the reaction of chlorine with water. Write an equation for the reaction of chlorine with hot NaOH. Bleach is used as a cleaning product to kill bacteria. It is made by adding compounds like sodium chlorate(, NaCl O, to water. Identify the formula of the ion present in bleach that kills bacteria. Sodium chlorate(, NaCl O, reacts with hydrogen peroxide to produce sodium chloride, water and oxygen gas. Construct an equation for this reaction. A sample of bleach W contains an unknown concentration of sodium chlorate(. 10.0 cm3 of W is diluted with distilled water to make a total volume of 100 cm3 of bleach solution. 25.0 cm3 of this diluted bleach solution is added to an excess of hydrogen peroxide and the volume of gas produced measured under room conditions. The experiment is repeated and on average 25.0 cm3 of diluted bleach solution produces 42.0 cm3 of gas. Calculate the concentration, in g dm–3, of sodium chlorate(in W. concentration of NaCl O in W = g dm–3
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THEORY
2023
Paper 2, Variant 2
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Nitrosyl chloride, NOCl, can be formed by the reaction between nitrogen monoxide and chlorine, as shown. 2NO + Cl 2 2NOCl The initial rate of this reaction is investigated, starting with different concentrations of NO and Cl 2. The results obtained are shown in Table 5.1. Table 5.1 experiment / mol dm–3 [Cl 2] / mol dm–3 initial rate / mol dm–3 min–1 0.0250 0.0150 3.68 × 10–2 0.0750 0.0150 3.32 × 10–1 0.0500 0.0600 5.89 × 10–1 Use the data in Table 5.1 to deduce the rate equation for this reaction. Explain your reasoning. Use your rate equation from and the data from experiment 1 to calculate the rate constant, k, for this reaction. Include the units of k. k = units NO2Cl is another compound containing nitrogen, oxygen and chlorine. In sunlight, NO2Cl can undergo homolytic fission to release chlorine radicals which can catalyse the conversion of ozone, O3, into oxygen. Complete the mechanism for this process. initiation (homolytic fission) NO2Cl + propagation step 1 + O3 + propagation step 2 + + Ozone reacts with nitrogen dioxide, as shown. O3 + 2NO2 N2O5 + O2 The rate of reaction is first order with respect to O3 and first order with respect to NO2. Suggest equations for a two‑step mechanism for this reaction. step 1 step 2 ,  ,
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THEORY
2024
Paper 4, Variant 2
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