remain after the reaction comes to an end. An understanding of chemical equilibrium and how it can be manipulated is essential for anyone involved in Chemistry and its applications. Iron-Silver Equilibrium In the first phase of the experiment‚ iron sulfate was mixed with silver nitrate‚ and the reaction produced solid silver and iron nitrate‚ which is formally written as Fe2+ (aq) + Ag+ (aq) ⇄ Ag (s) + Fe3+ (aq) It has a net equation of: Fe2+ (aq) + Ag+(aq) ↔ Fe3+(aq) + Ag(s) The mixture was then
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UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education *8621469522* COMBINED SCIENCE CO-ORDINATED SCIENCES Paper 6 Alternative to Practical 0653/06 0654/06 May/June 2009 1 hour Candidates answer on the Question paper No Additional Materials are required. READ THESE INSTRUCTIONS FIRST Write your Centre number‚ candidate number and name on all the work you hand in. Write in dark blue or black pen. You may use a soft pencil for any diagrams‚ graphs
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(constant) ∙mass of reactant used (mass is less that 3g) When we consider a double displacement reaction; we will need to think about the solubility rules. In our experiment we consider the rule that "Most nitrate (NO3-) salts are soluble." And "Most sulfate are soluble. Notable exceptions are BaSO4......" By this rules we can check the solutions that we will use during the experiment that whether it is soluble or not. Also‚ we can check after the reaction‚ which of the compound is the precipitate. Hence
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passed through them. For electrolysis to work‚ the ions must be free to move. Ions are free to move when an ionic substance is dissolved in water or molten (melted). For example‚ if electricity is passed through copper chloride solution‚ the copper chloride is broken down to form copper metal and chlorine gas. Here is what happens during electrolysis: Positively charged ions move to the negative electrode during electrolysis. They receive electrons and are reduced. Negatively charged ions move
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* Evaporating dish * Candle * Matches * Ammonium hydroxide * Watch glass * Phenolphthalein * Paper towel * Cornstarch * Iodine * Cup * Alka-Seltzer tablet * Pipet * Milk * Vinegar * Copper II sulfate * Lead II nitrate Safety: * Goggles were worn. * Aprons were worn. * Lab station was cleaned up directly following experiments. * Hands were washed after experiments. * No eating or drinking took place in the lab.
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In the project‚ four different chemicals will be used to change the color of the fire. The compounds are Sodium Chloride‚ Boric acid‚ Strontium Chloride‚ and Copper Sulfate. Two of the chemicals are metals and two are not. Sodium Chloride and Strontium Chloride are both metals. Boric Acid and Copper Sulfate are not‚ even though Copper sulfate is commonly mistaken as
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Guess Paper – 2009 Class – X Subject – Chemistry (P- Block Elements) Kalra sir 09460472649 kalra1977@rediffmail.com Group 15 elements: |Symbol |Atomic |Electronic configuration | | |number | | | |7 |[He]2s22p3 | |N | | | |P |15 |[Ne] 3s23p3 | |As |33 |[Ar]3d104s24p3
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fiber? 5. Which plant extract when combined with copper sulfate is suitable for dyeing cotton? 6. Does the acidity-basicity of the dye solution affect the quality of the dyed product? What you need Dye materials: plant parts such as peelings of mangosteen fruit‚ purple camote‚ and eggplant or red mayana and pandan leaves Fabrics: cotton‚ rayon‚ or any synthetic fiber Mordants: alum‚ copper sulfate‚ iron (II) sulfate‚ sodium sulfate 500-mL beaker stirring rods tray Masking tape
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Chemical Earth. 1. What is the systematic name for a compound with the formula Cu2SO4? (A) (B) (C) (D) 3. In which compound do all atoms have the same electronic configuration? (A) (B) (C) (D) 4. Copper sulfide Copper (I) sulfate Copper (II) sulfate Copper disulfate LiF NaCl MgF2 NCl3 Identify the property which decreases across each row of the Periodic Table. (A) (B) (C) (D) Melting point Ionisation energy Valency Atomic radius 11. Which is correct
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For the seventh experiment we will be performing different type of test to see how different chemical react with each other. The first experiment will be a demonstration the professor will give to the class. the first experiment you will be performing will include a test tube you will add a couple drops of dilute hydrochloric. you will add this to five little pieces of zinc metal. In next experiment you will performed you will put 2 ml of 3% hydrogen peroxide solution in a test tube .you will also
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