MFM2P1 - Mr. Tjeerdsma
... The ratios 6:9, 12:18, 18:27, 2:3 are all equivalent to one another. The ratio 2:3 is in lowest terms because it cannot be changed to an equivalent ratio using whole numbers by dividing both terms by the same number. ...
... The ratios 6:9, 12:18, 18:27, 2:3 are all equivalent to one another. The ratio 2:3 is in lowest terms because it cannot be changed to an equivalent ratio using whole numbers by dividing both terms by the same number. ...
5 Thermochemistry
... The book’s potential energy is due to the opposition of gravity by an object of mass m at a distance d above the surface of the earth. Kinetic energy is due to the motion of the book. As the book falls, d decreases and potential energy changes into kinetic energy. The first law states that the total ...
... The book’s potential energy is due to the opposition of gravity by an object of mass m at a distance d above the surface of the earth. Kinetic energy is due to the motion of the book. As the book falls, d decreases and potential energy changes into kinetic energy. The first law states that the total ...
Pre- AP & NET IONIC EQUATIONS
... Over the past 10 years the number of truly difficult non-trival reactions has dwindled. There have only been 2 and those were in years when you could easily have avoided them by choosing other options. Now that there are no options and reactions must be balanced it is questionable whether these kin ...
... Over the past 10 years the number of truly difficult non-trival reactions has dwindled. There have only been 2 and those were in years when you could easily have avoided them by choosing other options. Now that there are no options and reactions must be balanced it is questionable whether these kin ...
Chemical Energy
... /2N2(g) + O2(g) - NO2(g) Ho = 34 kJ/mol Mg(s) + 1/2O2(g) - MgO(s) Ho = -602 kJ/mol 2 P(s) + 3 Cl2(g) - 2 PCl3(s) Ho = -640 kJ/mol 2 P(s) + 5 Cl2(g) - 2 PCl5(s) Ho = -880 kJ/mol C(graphite) + 2 O(g) - CO2(g) Ho = -643 kJ/mol C(graphite) + O2(g) - CO2(g) Ho = -394 kJ/mol C(graphite) + 2 H2(g) - ...
... /2N2(g) + O2(g) - NO2(g) Ho = 34 kJ/mol Mg(s) + 1/2O2(g) - MgO(s) Ho = -602 kJ/mol 2 P(s) + 3 Cl2(g) - 2 PCl3(s) Ho = -640 kJ/mol 2 P(s) + 5 Cl2(g) - 2 PCl5(s) Ho = -880 kJ/mol C(graphite) + 2 O(g) - CO2(g) Ho = -643 kJ/mol C(graphite) + O2(g) - CO2(g) Ho = -394 kJ/mol C(graphite) + 2 H2(g) - ...
Empirical and Molecular Formulas.studentsdoc
... Step 2: Determine simplest ratio by dividing the lowest amount of moles determined in step 1 3.390/3.390 = 1 mol of C 5.04/3.390 = 1.5 mol of H 3.390/3.390 = 1 mol of O Then look at the three numbers of moles and determine the lowest number they can be multiplied by to get all whole numbers. In this ...
... Step 2: Determine simplest ratio by dividing the lowest amount of moles determined in step 1 3.390/3.390 = 1 mol of C 5.04/3.390 = 1.5 mol of H 3.390/3.390 = 1 mol of O Then look at the three numbers of moles and determine the lowest number they can be multiplied by to get all whole numbers. In this ...
Name - Beals Chemistry
... 1) What is the mass of one mole of arsenic? ____________________ 2) How many atoms are in one mole of arsenic? ____________________ 3) How many moles are contained in 2.005 x 1023 atoms of arsenic? _______________ 4) How many moles are in 200.5 grams of arsenic? ________________ 5) What is the formu ...
... 1) What is the mass of one mole of arsenic? ____________________ 2) How many atoms are in one mole of arsenic? ____________________ 3) How many moles are contained in 2.005 x 1023 atoms of arsenic? _______________ 4) How many moles are in 200.5 grams of arsenic? ________________ 5) What is the formu ...
Energy is the essence of chemistry It determines which reaction can
... CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ∆H ro = –890 kJ/mol -Pure CH4 gas at 1 atm. reacts with pure O2 gas at 1 atm. to form: -pure CO2 gas and water liquid at 1 atm. ...
... CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ∆H ro = –890 kJ/mol -Pure CH4 gas at 1 atm. reacts with pure O2 gas at 1 atm. to form: -pure CO2 gas and water liquid at 1 atm. ...
Chemistry 140
... Suggest the steps needed to find the solution. Develop a “roadmap” solution. 3)Solution: Calculations appear in the same order as outlined. ...
... Suggest the steps needed to find the solution. Develop a “roadmap” solution. 3)Solution: Calculations appear in the same order as outlined. ...
+ H 2 O(l)
... • Determining the concentration of an unknown solution. • Use a 2nd solution of known concentration (standard solution) that undergoes a reaction with the unknown solution. • Use the ratios in the balanced equation along with the M = mol/L equation to determine molarity of unknown. ...
... • Determining the concentration of an unknown solution. • Use a 2nd solution of known concentration (standard solution) that undergoes a reaction with the unknown solution. • Use the ratios in the balanced equation along with the M = mol/L equation to determine molarity of unknown. ...
Chapter 18 - Louisiana Tech University
... 7. Describe the connection between enthalpy and entropy changes for a reaction and the Gibbs free energy change; use this relation to estimate quantitatively how temperature affects whether a reaction is product-favored (Section 18.6). 8. Calculate the Gibbs free energy change for a reaction from va ...
... 7. Describe the connection between enthalpy and entropy changes for a reaction and the Gibbs free energy change; use this relation to estimate quantitatively how temperature affects whether a reaction is product-favored (Section 18.6). 8. Calculate the Gibbs free energy change for a reaction from va ...
Paper - Revision Science
... A benzene to produce an electrophile. B benzene to produce a nucleophile. C chloromethane to produce a nucleophile. D chloromethane to produce an electrophile. (Total for Question 13 = 1 mark) 14 The reaction below can be catalysed by either Fe2+ ions or Fe3+ ions. S2O82 –(aq) + 2I–(aq) ĺ 2SO42–(aq) ...
... A benzene to produce an electrophile. B benzene to produce a nucleophile. C chloromethane to produce a nucleophile. D chloromethane to produce an electrophile. (Total for Question 13 = 1 mark) 14 The reaction below can be catalysed by either Fe2+ ions or Fe3+ ions. S2O82 –(aq) + 2I–(aq) ĺ 2SO42–(aq) ...
Reporting Category 3: Bonding and Chemical Reactions
... How can you apply metallic bonding theory to explain metallic properties? The nature of metallic bonding explains many physical properties of metals. For example, most metals are excellent conductors of thermal energy. When a difference in thermal energy is applied across a metal, it is quickly and ...
... How can you apply metallic bonding theory to explain metallic properties? The nature of metallic bonding explains many physical properties of metals. For example, most metals are excellent conductors of thermal energy. When a difference in thermal energy is applied across a metal, it is quickly and ...
Press here to hemy 102 lab manual
... electron for each positive charge. 2- Write the symbols for the atoms to show which atoms are attached to which, and connect them with a single bond (a dash, representing two electrons). Chemical formulas are often written in the order in which the atoms are connected to the molecule or ion, as in H ...
... electron for each positive charge. 2- Write the symbols for the atoms to show which atoms are attached to which, and connect them with a single bond (a dash, representing two electrons). Chemical formulas are often written in the order in which the atoms are connected to the molecule or ion, as in H ...
AP Chemistry - Oak Park Unified School District
... Measurements are made using the metric system, where the standard units are called (4) units, which are based on the meter, kilogram, and second as the basic units of length, mass, and time, respectively. The SI temperature scale is the (5) scale, although the (6) scale is frequently used in chemist ...
... Measurements are made using the metric system, where the standard units are called (4) units, which are based on the meter, kilogram, and second as the basic units of length, mass, and time, respectively. The SI temperature scale is the (5) scale, although the (6) scale is frequently used in chemist ...
chemical change
... For each of the examples in (a) to (c) above, calculate the number of formula units, and the number of atoms of each element. CONVERTING MOLES OF SUBSTANCE TO MASS A chemist calculates that in a certain reaction, she has prepared 0.011 moles of zinc iodide, what is the mass of product produced? APPL ...
... For each of the examples in (a) to (c) above, calculate the number of formula units, and the number of atoms of each element. CONVERTING MOLES OF SUBSTANCE TO MASS A chemist calculates that in a certain reaction, she has prepared 0.011 moles of zinc iodide, what is the mass of product produced? APPL ...
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.