Chemistry Final Study Guide Matter as anything that has mass and takes up space. Significant figures refers to digits that were measured. When rounding calculated numbers‚ we pay attention to significant figures so we do not overstate the accuracy of our answers. Rules: -All nonzero digits are significant. -Zeroes between two significant figures are themselves significant. -Zeroes at the beginning of a number are never significant. -Zeroes at the end of a number are significant if a decimal
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5. What is a precipitate? It is a product of a reaction thats is insoluble and separates from a homogenous mixture as a solid. 6. Balance these equations: KBrO3(s)--------> KBr(s) + O2(g) Balanced: 2KBrO3(s)--------> 2KBr(s) + 3O2(g) MnBr2(aq) + AgNO3(aq) --------> Mn(NO3)2(aq) + AgBr(syou Balanced:MnAg2(aq) + 2AgNO3(aq) --------> Mn(NO3)2(aq) +2AgBr(s) 7. How could you distinguish between the gases H2 and NO2? H2is a colorless‚ odorless gas while NO2 has a reddish-brown
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Chemistry AP Chapters 4 and 5 Practice Test 1. Which of these compounds is a weak electrolyte? A. HCl B. CH3COOH (acetic acid) C. C6H12O6 (glucose) D. O2 E. NaCl 2. The balanced net ionic equation between aqueous diethyl ammonium chloride and aqueous potassium hydroxide contains which of the following species? A. KCl(s) B. 2 OH-1 C. (CH3CH2)2NH2 (aq) D. H3O+1 E. (CH3CH2)2NH2+1 (aq) 3. In the chemical reaction 5H2O2 + 2MnO4-
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Basic Requirements 1. Your project must be multimedia‚ containing both text and visual components and perhaps audio (visual means everything from photos to drawings to paintings to textiles to a slide show presentation to video; the possibilities are endless!). 2. Your project must describe important moments of your history. 3. Your project must be both symbolic and literal; you must include both direct descriptions about yourself‚ like those Esperanza shared‚ and include artwork that shows
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components of mixture of sand (SiO2)‚ salt (NaCl)‚ and chalk (CaCO3). 1. CaCO3+2HCl-----CaCl2+CO2+H2O 2. CaCl2+K2CO3====CaCO3+2KCl The first reaction shows the separation of calcium carbonate from the mixture. In the second reaction we use the product of the first reaction (CaCl2) and change it back to calcium carbonate (CaCO3) by mixing CaCl2 with potassium chloride (2KCl). Objective To separate the components of mixture of sand‚ sodium chloride and calcium carbonate. Materials and Equipment 1.
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SCORE SCIENCE 10 ONE MARK MODEL QUESTION PAPER CHAPTERWISE Compiled By‚ A. JEBASINGH‚ M. Sc.‚ M.Ed.‚ M.Phil. BT Asst. (Science) Edited By‚ A. SAVARIMUTHU‚ B.Sc.‚ M.A.(Eng).‚ B.Ed. BT Asst. (Science) Typed By‚ J. LOGESH OUR SINCERE THANKS TO Rev. Bro. Dr. M.IRUDHAYAM M.Sc.(Phy).‚ M.Sc.(E&E)‚ M.Sc.(Psy).‚ M.A.(Eng).‚ M.Phil.‚ M.A.(Soc).‚ M.Phil.‚ PGDCA‚ PGDHET‚ PGDEA‚ MBA‚ M.Ed.‚ PhD. HEADMASTER & CORRESPONDENT ST. JOSEPH’S HR. SEC. SCHOOL CHENGALPATTU- 603002 CONTACT
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Chemistry 11 Final Examination Review - Answers Part A - True or False. Indicate whether each of the following statements is true or false. Correct the false statements. F 1. The mass of an electron is equal to the mass of a proton. The mass of an electron is less than the mass of a proton. T 2. The mass of a proton is approximately equal to the mass of a neutron. T 3. The atomic number represents the number of protons in a nucleus. T 4. The proton has a mass of approximately
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attraction means that the required heat energy to reach the boiling point increases. Fluorine has a significantly lower boiling point than the rest of the halides because it has a set of electrons that produces repulsion between them. This weakens the bond. Chlorine has a boiling point of -34.6°C because its covalent bond is stronger than fluorine’s and so on until Iodine which has a boiling point of 184.0°C because it has many more energy levels which requires more heat energy. As the intermolecular
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the percentage uncertainty of alcohol burned moles percentage uncertainty of alcohol burned mass+percentage uncertainty of alcohol`s molar mass Calculating ΔH (enthalpy change) ΔH=-mass of water x specific heat of water x Δ T of water mol of alcohol * The specific heat for water is 4.18 =100x4.184x 10=4‚184 J or 4‚184 KJ exothermic Methanol= * H2O = 100 ml *
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energy. Planning We will be using 6 different fuels to heat up 100ml of water‚ and find out the changes of the temperature. We will measure the temperatures of the water before and after the experiment. We will burn heat the water for exactly 2 minutes‚ and check the changes in temperature. The change in temperature will allow us to work out the energy given off the fuel by using this formula: Mass of water x 4.2 (water’s specific heat capacity) x temperature change = energy transferred from
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