Inorganic Nomenclature I. Compound Type Fixed Charge Metal Binary Salts Description Fixed Charge Metal* + a Nonmetal Rule: Full name of the metal + Stem on the nonmetal + the suffix “ide” Formula Name NaCl Sodium chloride CsF Cesium fluoride CaBr2 Calcium bromide MgO Magnesium oxide Li2S Lithium sulfide Al2O3 Aluminum oxide ZnH2 Zinc hydride AgI Silver iodide SrS Strontium sulfide Ca3N2 Calcium nitride K2Te Potassium telluride Na3N Sodium nitride CaC2 Calcium carbide LiH Lithium hydride Mg3P2 Magnesium
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Experiment 1: Calorimetry Nadya Patrica E. Sauza‚ Jelica D. Estacio Institute of Chemistry‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines Results and Discussion Eight Styrofoam ball calorimeters were calibrated. Five milliliters of 1M hydrochloric acid (HCl) was reacted with 10 ml of 1M sodium hydroxide (NaOH) in each calorimeter. The temperature before and after the reaction were recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature
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6. To study the rate constant in the rate equation of 2 I- + S2 O82- I2 + 2 SO42-. Results: Table 1: Volume of reactants (S2O82-‚ [NH4]2 SO4‚ I-‚ KNO3) added and the concentration of the reactants (S2O82-‚ I-). Experiment Volume of 0.20M (S2O82-) Volume of 0.20M [NH4]2 SO4 Volume of 0.20M (I-) Volume of 0.20M KNO3 Temperature Concentration of (S2O82-) Concentration of (I-) A i. 25cm3 - 25cm3 - RT *0.20M 0.20M ii. 25cm3 75cm3 25cm3 - RT **0.05M 0
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shift that closes an electrical contact‚ telling the sensors that a crash has occurred. The sensors receive information from an accelerometer built into a microchip. The airbag ’s inflation system reacts sodium azide (NaN3) with potassium nitrate (KNO3) to produce nitrogen gas. Hot blasts of the nitrogen inflate the
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2NH4+ (aq.) Pb2+(aq.)+2Cl- (aq.) ---- PbCl2(s) Pb2+(aq.)+2OH-(aq.) ----Pb(OH)2 (s) Pb2+(aq.)+ 2NH3(aq.)+ H2O(l) --- Pb(OH)2 (s)+ 2NH4+ (aq.) Cu2+(aq.) +2OH-(aq.) ---- Cu(OH)2 (s) 2Cu2+(aq.)+SO42- (aq.) +2NH3(aq.)+2 H2O(l) ----- Cu(OH)2.CuSO4(s) +2NH4+ (aq.) Zn2+ (aq.)+ 2OH- (aq.) ---- Zn(OH)2 (s) Zn2+ (aq.)+2NH3(aq.)+ H2O(l) --- Ag2O (s)+ 2NH4+ (aq.) Fe3+ (aq.)+ 3OH- (aq.) ---- Fe(OH)3(s) Fe3+ (aq.)+ 3NH3(aq.)+ 3H2O(l) --- Fe(OH)3(s)+ 3NH4+ (aq.) Pb2+(aq.)+ CrO42-(aq.)
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Test Reagent Observation Fe2+ 0.10M K3Fe(CN)6 Prussian blue precipitate Fe 3+ 0.10 M KSCN Blood red solution Ag+ 1.00 M HCl White precipitate Copper (II) – Ammonia System 1.00 M NH3 was added dropwise to a test tube filled with 1ml of 0.1 M CuSO4. Contents were mixed after each drop‚ and the number of drops needed to form precipitate and the additional drops needed to dissolve to precipitate were counted. Chromate – Dichromate System Four wells of a clean spot plate was labeled 1‚ 2‚ 3‚
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Muhil Arumugam Gold 3 Calculating the Formula of a Hydrate through Experimentation Purpose The purpose of this lab is to determine the formula of a given hydrate through collecting and calculating experimental data. Data Mass (g) of crucible 29.9g Mass (g) of crucible with hydrate 32.35g Mass (g) of crucible and anhydrous salt 31.39g Questions and Calculations 1. What was the mass of the original hydrate? 2.45g of hydrate Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible
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Observation of Chemical Changes Purpose In this experiment‚ the student studied the composition of materials in a setting where the indications of chemical changes were safely observed. The changes observed consisted of bubble formation‚ colors‚ viscosity‚ and precipitate formation. Procedure Using a well plate: use a different well for each chemical combination. Two drops (unless otherwise noted) of each chemical in the combinations (below) should be placed in one well. A dark and light
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Liquid mixture appears to thicken when mixed K NH3 and CuSO4 Two clear liquids turn to pearly blue when mixed Observations from procedure: BTB remains blue when exposed to a base and turns yellow when exposed to an acid. Phenolphthalein turns grey when exposed to a base and pink when exposed to an acid.
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2011 1. Upon the addition of potassium nitrate to liquid water‚ the beaker feels cold. Explain‚ using appropriate terms: system‚ surroundings‚ heat‚ temperature‚ endothermic or exothermic. The endothermic process whereby the system of KNO3 crystals dissolving in the water absorb energy from the surroundings and the measured temperature of the surroundings (beaker‚ air) drops. 2. The phase change from a gas to a liquid is called condensation. Is the enthalpy change‚ g
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