Redox Problem Set 1: Reactions and Stoichiometry (All of these questions are no calculator friendly) 1) Give the oxidation number of carbon in each of the following: a) b) c) d) CF2Cl2 Na2C2O4 HCO3-1 C2H6 2) Give the oxidation number of sulphur in each of the following: a) b) c) d) SOCl2 H2S2 H2SO3 Na2S 3) Identify the oxidizing and reducing agents in each of the following: a) b) c) d) 8H+(aq) + 6Cl-1(aq) + Sn(s) + 4NO3-1(aq) SnCl6 -2(aq) + 4NO2(g) + 4H2O(l) 2MnO4-1(aq) + 10Cl-1(aq) + 16H+(aq)
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Battle et al [ ] concluded TN to be 278 ± 5 K from Massbauer and neutron diffraction studies on 57Fe doped SrMnO3 which value of TN was expected to be little different from that for undoped one. The variation of electrical conductivity with oxygen stoichiometry and the correlation of high temperature stability with structure were also reported by Battle et al [ ] besides others [ ‚ ]. The results of this synthesis and XRD characterization as well as measurement of SrO activities in this inter oxide
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Sr(NO3)2 b. Na2CO3 g. CuSO4 c. BaCl2 h. CuCl2 d. Al(OH)3 g. PbS e. Zn(CH3COO)2 6. Complete the following double replacement (exchange ) reactions. Be sure to balance them. a. MgCl2 + Ba(NO3)2 → b. Al2(CrO4)3 + (NH4)2SO4 → c. K2SO4 + SrCl2 → d. FeCl3 + KOH → e. HCl + AgNO3 → f. K2SO4 + Ba(NO3)2 → 7. (Brown 4.21) Will precipitation occur when the following solutions are mixed? If so‚ write a balanced chemical equation for the reaction. a. Na2CO3 and AgNO3
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The mass of CaCO3 needed was calculated using the ideal gas law and stoichiometry; the amount needed was 0.256 g of CaCO3. Three measurements of 0.256 g were used for three trials. Each trial‚ CaCO3 was placed into a tissue paper‚ and then tied off with a string to prevent the loss of CaCO3. The diameter and the length of the
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calorimeter. The heat capacity (Ccal) of each calorimeter was calculated using the formula‚ C_cal=(-〖∆H〗_rxn^o n_LR)/∆T [1] where ∆Horxn is the total heat absorbed or evolved for every mole of reaction and nLR is the number of moles of the limiting reactant. The ∆Horxn used was -55.8kJ per mole of water while the nLR was 0.005 mole. Table 1. Average Ccal from recorded ∆T values. Trial ∆T‚ (oC) Ccal‚ (J) Ave Ccal‚ (J) 1 1 2.2 126.82 202.91 2 1.0 279.00 2 1 3.0 93.00 108.50 2 2.3
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CHNG 1103 INTRODUCTION OF MATERIAL AND ENERGY TRANSFORMATIONS COURSE NOTES PART A: MATERIAL BALANCE GENERAL INFORMATION LECTURERS Dr. Marjorie Valix (Part A: Material Balance) email: mvalix@usyd.edu.au office: Rm 444 Chemical Engineering Blg. Phone: 93514995 (Direct) or 9351 2455 (General Office/Messages) Dr. Vincent Gomes (Part B: Energy Balance) Email: vgomes@usyd.edu.ua Office: Rm 452 Chemical Engineering Blg. Phone: 9351 4868 TEXTBOOK R.M. Felder and R.W. Rousseau “ Elementary
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Hydrogen Peroxide & Inorganic Peroxy Compounds Hydrogen Peroxide Hydrogen peroxide (H2O2) is the simplest peroxide (a compound with an oxygen-oxygen single bond). It is also a strong oxidizer. Hydrogen peroxide is a clear liquid‚ slightly more viscous than water. In dilute solution‚ it appears colorless. Reactions Decomposition Hydrogen peroxide decomposes exothermically into water and oxygen gas spontaneously: 2 H2O2 → 2 H2O + O2 This process is thermodynamically favorable. It has
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Title: Preparation and isolation of an Ester Aim: To make an ester and purify it Background Theory: Esters are derived from carboxylic acids and alcohols with the presence of a catalyst. A carboxylic acid contains the -COOH group‚ and in an ester the hydrogen in this group is replaced by a hydrocarbon group of some kind. Sulfuric acid (H2SO4)is used as a catalyst for this reaction in order to accelerate the rate at which the product is formed. The general formula of an ester is RCOOR’ in
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crystal was weighed. The melting point range of the recrystallized tin tetraiodide was measured using a MEL-TEMP. Instruments should be washed by acetone during the experimental. Result Table 1 contains the molar mass‚ mass and the moles of reagents (Sn and I2) and products (crude SnI4‚ recrystallized SnI4 and air-dry SnI4). The yields of product and percent recover of
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Lab Report: Stoichiometry Lab Oct. 27‚ 2011 Claire Elizabeth Lab Partners: Hannah Signature:___________________ Introduction- Baking soda and vinegar are two common materials found in almost every household. That‚ plus the fact that all the starting and finishing materials are non hazardous and safe‚ is why this is one of the first chemical reactions that many people are exposed to The purpose of this experiment tests which of the two reactants (vinegar and baking soda) is the limited
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