ml of 0.01mol L-1 KMnO4 to 2 ml of 2mol L-1 H2SO4 3) Add 1 ml of this acidified KMnO4 solution to each of the test tubes containing the hydrocarbons. Shake each test tube gently and record any change that takes place in the aqueous layer over about 5 minutes. Reaction of hydrocarbons with bromine water: 1) Into three separate‚ labeled test tubes place 1 ml of cyclohexane‚ cyclohexene and toluene respectively. 2) Add 1 ml of bromine water to each of the test tubes containing the hydrocarbons
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Data-based questions Study the photos below and answer the following questions. Photo A Photo B Photo C (a) What are industries shown in photos A‚ B and C respectively? (3 marks) (b) Draw a diagram to illustrate the manufacturing system of the industry shown in photo A. (4 marks) (c) Describe and explain the characteristics of these three industries. (i) Photo A (3 marks) (ii) Photo B (3 marks) (iii) Photo C (in tradition) (3 marks) (d) How do personal factors affect
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Objectives The main objective of this experiment is to differentiate between a physical change and a chemical change. A physical change includes a change in the material without affecting its composition‚ such as the physical state change. However‚ a chemical change includes the change in the composition of the substance. The change in color‚ formation of a gas or a solid product‚ and the production of energy are the evidences of a chemical reaction‚ thus‚ of a chemical change. Materials
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common powders such as Alka-Seltzer‚ baking soda‚ flour‚ Vitamin C (ascorbic acid)‚ and salt. Other chemicals that were used to do this experiment were vinegar‚ and Iodine 2 Solution. The equipment used to do this experiment was red litmus paper‚ and 5 test tubes per group. After all materials were gathered‚ we then had to do five different tests to determine what the powder material does. The first test was to see what the powder materials do in water. We had to add a scoop of each of the common
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of an element [B: 10.01u] [B: 11.01u] 1) Given average atomic mass: 10.81u If given percentages‚ you can find average atomic mass by adding each portion 2) Set variables for unknown values Let x represent % abundance for 10/5 B Let 1-x represent % abundance for 11/5 B Calculate: 10.01x+(1-x)11.01=10.81 10.01x+11.01-11.01x=10.81 -1.00x=0.2 X=0.2 The Mole and Avogadro’s constant Mole: the SI unit that is used to measure how much of a substance. (balanced eqn coefficient are moles) Converting
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precautions All enzymes are potential allergens therefore eye and skin should be avoided Wear eye protection throughout the experiment and avoid rubbing eyes if the enzyme solution on hands in contact. Chemical Reagants Hydrogen peroxide solution (5-9 moldm-3) Materials / Equipment: Potato Cock Borer Test tube Knife Pipette Boiling tube Delivery tube Stopwatch Method: 1. 5.0cm3 of 2.0moldm-3 hydrogen peroxide solution is poured into tube 1. The bug is placed and followed by water
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concentration in the Dead Sea due to high evaporation and damaged aquatic life near the Great Barrier Reef caused by run-off from agricultural land. Eutrophication is caused by an excess amount of nitrate and phosphate in water bodies. It is usually caused by fertiliser run off and dumping of sewage going into waterways (basically human activity). Algal bloom is the direct result of eutrophication where suffocation of aquatic life and nutrient depletion may occur. Professionals may use a colorimetric
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solution and the alligator clips remain out of the solution. Note: The solution in the Petri dish top will serve as a control. 4. To start the demonstration‚ clip the 9-volt battery into the snaps on the battery cap (Figure 1). 5. Let the demonstration run for 5–10 minutes and note the changing colors over time and the production of gases (bubbling) at each electrode. A deep purple color forms immediately at the negative electrode‚ while at the positive electrode a red- orange color appears
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Chapter 4 - Chemical Bonding Outline • 4.2 Naming Compounds and Writing Formulas • 4.1 Types of Chemical Bonds • 4.4 Electronegativity‚ Unequal Sharing‚ and Polar Bonds • 4.5 Vibrating Bonds and the Greenhouse Effect • 4.3 Lewis Structures • 4.6 Resonance • 4.7 Formal Charge: Choosing among Lewis Structures • 4.8 Exceptions to the Octet Rule • 4.9 The Lengths and Strengths of Covalent Bonds © 2014 W. W. Norton Co.‚ Inc. 1 Chemical Bonds All chemical bonds consist of _______ that
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Leading zeros are not significant. Example: 0.000045 (2 sig. figs.) 5. Measured values that have trailing zeros only to the left of the decimal point are ambiguous and should be expressed in scientific notation. We must take note that the chemistry textbook (Silberberg 6e) states that placing a decimal point to the right of some trailing zeros (example: 300.) will make the zeros significant. However in General Chemistry‚ we do not follow this rule. If we want to write a whole number with trailing
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