with answers
... Foreign students may use a dictionary (mother tongue – English) but this may not contain any handwritten notes. The use of a calculator is not permitted. Numerical answers that are given without showing any working or explanation will receive no marks. In general, short answers with keywords will be ...
... Foreign students may use a dictionary (mother tongue – English) but this may not contain any handwritten notes. The use of a calculator is not permitted. Numerical answers that are given without showing any working or explanation will receive no marks. In general, short answers with keywords will be ...
Unit 2
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
Unit 2
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
... a) which elements are metals? _____________________________________ b) which elements are nonmetals? ___________________________________ c) which elements are metalloids? ___________________________________ 25) A compound has two boron atoms and six hydrogen atoms. a) what is its empirical formula? ...
Paper
... 7. A chemical equilibrium is established when eleven moles of hydrogen and eleven moles of iodine are mixed at a temperature of 764 K. Initially the colour of the mixture is deep purple due to the high concentration of iodine vapour. The purple colour fades and when equilibrium is established the co ...
... 7. A chemical equilibrium is established when eleven moles of hydrogen and eleven moles of iodine are mixed at a temperature of 764 K. Initially the colour of the mixture is deep purple due to the high concentration of iodine vapour. The purple colour fades and when equilibrium is established the co ...
Part II - American Chemical Society
... b. Would the A factor for the chemical reaction NO(g) + N2O(g) → NO2(g) + N2(g) be expected to be larger or smaller than the A factor in the above reaction if each reaction occurs in a single step? Outline your reasoning. c. Calculate the rate constant for this reaction at 75 ˚C. d. The following tw ...
... b. Would the A factor for the chemical reaction NO(g) + N2O(g) → NO2(g) + N2(g) be expected to be larger or smaller than the A factor in the above reaction if each reaction occurs in a single step? Outline your reasoning. c. Calculate the rate constant for this reaction at 75 ˚C. d. The following tw ...
Question 2
... 1. Small quantities of hydrogen gas can be prepared in the laboratory by the following reaction: Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) Assume you carried out this experiment and collected 653 mL of hydrogen gas over water. The gas mixture collected includes hydrogen and water vapor. The temperature ...
... 1. Small quantities of hydrogen gas can be prepared in the laboratory by the following reaction: Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) Assume you carried out this experiment and collected 653 mL of hydrogen gas over water. The gas mixture collected includes hydrogen and water vapor. The temperature ...
Chapter 7
... • K + Br2 → KBr • K + Br2 → 2KBr • First I add a 2 to the product to end with 2 bromine atoms, but now I am also ending with 2 potassium atoms. • 2K + Br2 → 2KBr • Adding a 2 in front of potassium fixes this. ...
... • K + Br2 → KBr • K + Br2 → 2KBr • First I add a 2 to the product to end with 2 bromine atoms, but now I am also ending with 2 potassium atoms. • 2K + Br2 → 2KBr • Adding a 2 in front of potassium fixes this. ...
A Thumbnail Review of Regents Chemistry
... ppm = (mass of solute / mass of solution) x 1,000,000 TABLE F is used to determine which IONIC SOLUTES are soluble in water TABLE G is used to determine if aqueous solutions are saturated, unsaturated or supersaturated KINETICS & EQUILIBRIUM The more effective collisions, the faster the reaction rat ...
... ppm = (mass of solute / mass of solution) x 1,000,000 TABLE F is used to determine which IONIC SOLUTES are soluble in water TABLE G is used to determine if aqueous solutions are saturated, unsaturated or supersaturated KINETICS & EQUILIBRIUM The more effective collisions, the faster the reaction rat ...
200 ways to pass the regents
... 108. Molarity is a way to measure the concentration of a solution. Molarity is equal to the number of moles of solute divided by the number of liters of solution. The formula is on the back of the reference tables. 109. Percent by mass = mass of the part / mass of the whole x 100% 110. Parts per mil ...
... 108. Molarity is a way to measure the concentration of a solution. Molarity is equal to the number of moles of solute divided by the number of liters of solution. The formula is on the back of the reference tables. 109. Percent by mass = mass of the part / mass of the whole x 100% 110. Parts per mil ...
New Title
... a. H2 + O2 H2O b. Mg + O2 MgO c. Na + O2 Na2O d. 2 H2O2 2 H2O + O2 17. A number placed in front of a chemical formula in a chemical equation is called a(n) 18. What does a coefficient tell you? ...
... a. H2 + O2 H2O b. Mg + O2 MgO c. Na + O2 Na2O d. 2 H2O2 2 H2O + O2 17. A number placed in front of a chemical formula in a chemical equation is called a(n) 18. What does a coefficient tell you? ...
Chapter 3
... A chemical reaction will change the arrangements of atoms in substances; but it neither destroy nor create atoms (matter) because of the reaction. The quantitative nature of chemical reactions arises from the law of conservation of matter. © 2012 by W. W. Norton & Company ...
... A chemical reaction will change the arrangements of atoms in substances; but it neither destroy nor create atoms (matter) because of the reaction. The quantitative nature of chemical reactions arises from the law of conservation of matter. © 2012 by W. W. Norton & Company ...
1 mole = 6.02 X 10 23 Particles
... One mole of $1 bills stacked one on top of another would reach from the Sun to Pluto and back 7.5 million times. It would take light 9500 years to travel from the bottom to the top of a stack of 1 mole of $1 bills. ...
... One mole of $1 bills stacked one on top of another would reach from the Sun to Pluto and back 7.5 million times. It would take light 9500 years to travel from the bottom to the top of a stack of 1 mole of $1 bills. ...
Chemistry - Edexcel
... centre number and candidate number. all questions. t Answer the questions in the spaces provided t Answer – there may be more space than you need. Show all the steps in any calculations and state the units. t Some questions must be answered with a cross in a box t your mind about an answer, put a li ...
... centre number and candidate number. all questions. t Answer the questions in the spaces provided t Answer – there may be more space than you need. Show all the steps in any calculations and state the units. t Some questions must be answered with a cross in a box t your mind about an answer, put a li ...
Review Unit - hrsbstaff.ednet.ns.ca
... A reaction between two chemicals dissolved in water is shown three ways: i. Molecular Equation - the reaction is written as if all of the chemicals consist of ...
... A reaction between two chemicals dissolved in water is shown three ways: i. Molecular Equation - the reaction is written as if all of the chemicals consist of ...
Chemistry EOC Review
... 325mm Hg to 550mm Hg, what is the new volume of the gas? 80) A sample of gas has a volume of 140.0mL at 67C. To what temperature must the gas be lowered to reduce its volume to 50.0 mL at constant pressure? 81) A sample of gas at 47C and 780.mm Hg pressure occupies a volume of 2.20L. What volume w ...
... 325mm Hg to 550mm Hg, what is the new volume of the gas? 80) A sample of gas has a volume of 140.0mL at 67C. To what temperature must the gas be lowered to reduce its volume to 50.0 mL at constant pressure? 81) A sample of gas at 47C and 780.mm Hg pressure occupies a volume of 2.20L. What volume w ...
1 1. Give two reasons why a luminous flame is not used for heating
... a) What is observed when hydrogen sulphide gas is bubbled into lead II nitrate solution? 1mk b) Write an ionic equation for the reaction. 1mk*UG* The table below shows the solubility of potassium nitrate and potassium chlorate at various temperatures Salt Solubility at various temperatgure 500C 200C ...
... a) What is observed when hydrogen sulphide gas is bubbled into lead II nitrate solution? 1mk b) Write an ionic equation for the reaction. 1mk*UG* The table below shows the solubility of potassium nitrate and potassium chlorate at various temperatures Salt Solubility at various temperatgure 500C 200C ...
CHEM 1A General Chemistry I (1)
... This course introduces atomic structure, bonding, stoichiometry, thermochemistry, gases, matter and energy, oxidation-reduction, chemical equations, liquids and solids, solutions, chemical energetics and equilibrium. The first semester of a one-year course in chemistry intended for majors in the nat ...
... This course introduces atomic structure, bonding, stoichiometry, thermochemistry, gases, matter and energy, oxidation-reduction, chemical equations, liquids and solids, solutions, chemical energetics and equilibrium. The first semester of a one-year course in chemistry intended for majors in the nat ...
Classification of Matter
... The arrow means yields (makes) C + O2 CO2 (products) Reactants (yield) products ...
... The arrow means yields (makes) C + O2 CO2 (products) Reactants (yield) products ...
AP Chemistry Summer Study Guide
... 5.00 grams of ethanol and an excess of aqueous potassium permanganate are reacted and 5.98grams of acetic acid results. What is the percent yield? If 45ml of a 1.50M AgNO3 solution is added to 25.0grams of NaCl, how many grams of AgCl can be produced? How many liters of a 3.0M phosphoric acid soluti ...
... 5.00 grams of ethanol and an excess of aqueous potassium permanganate are reacted and 5.98grams of acetic acid results. What is the percent yield? If 45ml of a 1.50M AgNO3 solution is added to 25.0grams of NaCl, how many grams of AgCl can be produced? How many liters of a 3.0M phosphoric acid soluti ...
Chapter 2: Mass Relations in Formulas, Chemical Reactions, and
... present in the least number of compounds. In the above equation, we can start with either carbon or hydrogen. Balancing the element carbon. There is one carbon atom on the left-hand side (in CO2(g)) and six carbon atoms on the right-hand side (in C6H12O6(s)). Hence, we place a coefficient of 6 in fr ...
... present in the least number of compounds. In the above equation, we can start with either carbon or hydrogen. Balancing the element carbon. There is one carbon atom on the left-hand side (in CO2(g)) and six carbon atoms on the right-hand side (in C6H12O6(s)). Hence, we place a coefficient of 6 in fr ...
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.