MULTIPLE CHOICE. Choose the one alternative that best completes
... E) are generally 100 or more times sweeter than sucrose. ...
... E) are generally 100 or more times sweeter than sucrose. ...
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... -There are 4 unpaired electrons. -Water is a weak ligand. Thus the hybridisation involved is sp3d2 (marks to be granted if hybridisation is depicted diagrammatically) (ii) The ionisation isomer is [Co(NH3)5SO4]Br. The IUPAC name is pentaamminesulphatocobalt(III)bromide. Chemical test to distinguish ...
... -There are 4 unpaired electrons. -Water is a weak ligand. Thus the hybridisation involved is sp3d2 (marks to be granted if hybridisation is depicted diagrammatically) (ii) The ionisation isomer is [Co(NH3)5SO4]Br. The IUPAC name is pentaamminesulphatocobalt(III)bromide. Chemical test to distinguish ...
chapter 3
... CHAPTER 3. STOICHIOMETRY Chemical equations describe chemical reactions. Common symbols: (g) or ↑ gas; ...
... CHAPTER 3. STOICHIOMETRY Chemical equations describe chemical reactions. Common symbols: (g) or ↑ gas; ...
Stoichiometry1
... and neutrons, so they have different masses (isotopes) Carbon-12 (6 p+, 6 no)has a mass 12 times greater than hydrogen-1(1 p+, 0 no) It’s impossible to measure the mass of individual atoms on a balance, because it is so small Chemists developed their own unit, called the mole ...
... and neutrons, so they have different masses (isotopes) Carbon-12 (6 p+, 6 no)has a mass 12 times greater than hydrogen-1(1 p+, 0 no) It’s impossible to measure the mass of individual atoms on a balance, because it is so small Chemists developed their own unit, called the mole ...
Knox Chem Prelim 2009
... White precipitates are formed when sodium hydroxide is added to magnesium chloride solution and when sulphuric acid is added to barium nitrate solution. Predict the result of adding together equal volumes of 0.05 mol/L barium hydroxide and magnesium ...
... White precipitates are formed when sodium hydroxide is added to magnesium chloride solution and when sulphuric acid is added to barium nitrate solution. Predict the result of adding together equal volumes of 0.05 mol/L barium hydroxide and magnesium ...
Pretest 4.3 2008
... a. In Period 2, electronegativity increases as the atomic number increases. b. In Period 2, ionization energy decreases as the atomic number increases. c. In Period 2, atomic radius does not change as the atomic number increases. d. In group 1 (alkali metals), boiling points decrease and then increa ...
... a. In Period 2, electronegativity increases as the atomic number increases. b. In Period 2, ionization energy decreases as the atomic number increases. c. In Period 2, atomic radius does not change as the atomic number increases. d. In group 1 (alkali metals), boiling points decrease and then increa ...
Mole/Stoich PowerPoint Notes
... • Ex: N2(g) + 3H2(g) ---> 2NH3(g) • This says that 1 molecule of N2 reacts with 3 molecules of H2 to give 2 molecules of NH3 gas. • Let’s say you have 1 mole of nitrogen gas and an unlimited supply of hydrogen gas – 1. How much of the hydrogen gas will react with the nitrogen gas? 3 moles – 2. How m ...
... • Ex: N2(g) + 3H2(g) ---> 2NH3(g) • This says that 1 molecule of N2 reacts with 3 molecules of H2 to give 2 molecules of NH3 gas. • Let’s say you have 1 mole of nitrogen gas and an unlimited supply of hydrogen gas – 1. How much of the hydrogen gas will react with the nitrogen gas? 3 moles – 2. How m ...
2016 - Specimen Paper 2 - Cambridge International Examinations
... 12 20 cm3 of ethyne, C2H2, are reacted with 500 cm3 of oxygen. The equation for the reaction is 2C2H2(g) + 5O2(g) ...
... 12 20 cm3 of ethyne, C2H2, are reacted with 500 cm3 of oxygen. The equation for the reaction is 2C2H2(g) + 5O2(g) ...
Stoichiometry: Calculations with Chemical Formulas and Equations
... grams of each element in 100 g of sample. 3. From these masses, calculate the number of moles (use atomic weight from Periodic Table) 4. The lowest number of moles becomes the divisor for the others. (gives a mole ratio greater than 1) 5. Adjust mole ratios so all numbers are whole (1, 2, etc) 6. Th ...
... grams of each element in 100 g of sample. 3. From these masses, calculate the number of moles (use atomic weight from Periodic Table) 4. The lowest number of moles becomes the divisor for the others. (gives a mole ratio greater than 1) 5. Adjust mole ratios so all numbers are whole (1, 2, etc) 6. Th ...
Chemical bonding
... Acetic Acid + sodium hydrogen carbonate sodium acetate + water + carbon dioxide RED= REACTANTS BLUE= PRODUCTS = YIELDS/PRODUCES ...
... Acetic Acid + sodium hydrogen carbonate sodium acetate + water + carbon dioxide RED= REACTANTS BLUE= PRODUCTS = YIELDS/PRODUCES ...
Aluminum and Copper
... 2. Cut a piece of aluminum foil approximately 6" × 12". Loosely roll the foil into a cylinder that will fit into the beaker. (Do not wad up the foil tightly into a ball.) 3. Place the aluminum foil into the beaker, using a stirring rod to push it down into the solution. 4. Observe the “sign ...
... 2. Cut a piece of aluminum foil approximately 6" × 12". Loosely roll the foil into a cylinder that will fit into the beaker. (Do not wad up the foil tightly into a ball.) 3. Place the aluminum foil into the beaker, using a stirring rod to push it down into the solution. 4. Observe the “sign ...
SCH 3U - mquagliaoths
... All of these questions have answers in the back of the textbook except for page 212 #42. So here is its answer: i) decomposition – a compound is broken down into smaller parts; only one reactant is present ii) synthesis – the opposite of decomposition in that 2 (or more) reactants come together to m ...
... All of these questions have answers in the back of the textbook except for page 212 #42. So here is its answer: i) decomposition – a compound is broken down into smaller parts; only one reactant is present ii) synthesis – the opposite of decomposition in that 2 (or more) reactants come together to m ...
Experiment 11 CHEMICAL REACTIONS
... A single replacement reaction will occur only if the element reacting is more “ active” than the element it is replacing. If the element reacting is a metal, it re places a metal (or hydrogen) in the compound. However, the reaction will occur only if a more active metal is replacing a less active me ...
... A single replacement reaction will occur only if the element reacting is more “ active” than the element it is replacing. If the element reacting is a metal, it re places a metal (or hydrogen) in the compound. However, the reaction will occur only if a more active metal is replacing a less active me ...
About writing chemical equations ppt
... Writing and Balancing Equations 5. The physical state of a substance is indicated by the following symbols: (s) solid (l) liquid (g) gaseous (aq) aqueous: means water solution yields reversible H2 ...
... Writing and Balancing Equations 5. The physical state of a substance is indicated by the following symbols: (s) solid (l) liquid (g) gaseous (aq) aqueous: means water solution yields reversible H2 ...
Compounds and Equations
... When chemical reactions take place, we can think about them as if they were recipes. These recipes are based on mole amount of each ingredient. However, we don’t have balances that measure moles, we always measure in grams. Therefore, we need to be able to convert between grams and moles of our ingr ...
... When chemical reactions take place, we can think about them as if they were recipes. These recipes are based on mole amount of each ingredient. However, we don’t have balances that measure moles, we always measure in grams. Therefore, we need to be able to convert between grams and moles of our ingr ...
Power point types of chemical rxn
... http://www.youtube.com/watch?v=_P5hGzA6Vb0 See page 263 (c) McGraw Hill Ryerson 2007 ...
... http://www.youtube.com/watch?v=_P5hGzA6Vb0 See page 263 (c) McGraw Hill Ryerson 2007 ...
PP1 - Swiftchem.org
... • Earlier, we found that the empirical formula of a compound was CH2O. • If we know the molecular mass of the compound is 180 g/mol, then we can determine the molecular formula. • We can calculate the mass of the empirical formula (CH2O). It is 30.0 g/mol • Next, we divide our molecular mass of the ...
... • Earlier, we found that the empirical formula of a compound was CH2O. • If we know the molecular mass of the compound is 180 g/mol, then we can determine the molecular formula. • We can calculate the mass of the empirical formula (CH2O). It is 30.0 g/mol • Next, we divide our molecular mass of the ...
Section 4.6: Double Displacement Reactions
... 7. Silver ions are the only metal ions that can be precipitated from a solution containing the C2H3O2− ions. Therefore, a solution such as NaC2H3O2(aq) can be used to precipitate silver ions from a mixture of dissolved metal ions. 8. Answers may vary. Sample answer: Most of the limescale that forms ...
... 7. Silver ions are the only metal ions that can be precipitated from a solution containing the C2H3O2− ions. Therefore, a solution such as NaC2H3O2(aq) can be used to precipitate silver ions from a mixture of dissolved metal ions. 8. Answers may vary. Sample answer: Most of the limescale that forms ...
Phy 211: General Physics I
... The number of sides on a square The number of apples on a desktop ...
... The number of sides on a square The number of apples on a desktop ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.