ACTIVATION ENERGY VARIATION DURING IGNITION OF
... occurrence. A very specific property characterizing the system is the induction period of the ignition and its dependence on the mixture pressure and composition as well as on the surface temperature [5y7]. The variation of this property on the system variables gives valuable information on the kine ...
... occurrence. A very specific property characterizing the system is the induction period of the ignition and its dependence on the mixture pressure and composition as well as on the surface temperature [5y7]. The variation of this property on the system variables gives valuable information on the kine ...
SCH3U Chemistry 11 Course Notes 2015
... 6. Calculate your group’s percent error using the equation & value on the board. ...
... 6. Calculate your group’s percent error using the equation & value on the board. ...
Ionic Equations
... soluble {except Pb(II), Ag(I) and Hg(I)} Carbonates and phosphates are generally insoluble (except group I) Hydroxides and sulphides are generally insoluble (except groups I and II) ...
... soluble {except Pb(II), Ag(I) and Hg(I)} Carbonates and phosphates are generally insoluble (except group I) Hydroxides and sulphides are generally insoluble (except groups I and II) ...
Final Exam Review Packet
... _____ 4. Benzene, C6H6, boils at 80.1˚C and has a density of 0.877 g/cm3. Determine the quantity of heat that is required to vaporize a 45.6 mL sample of benzene at 35.0˚C. a. 3140 J b. 4370 J c. 15800 J d. 18900 J _____ 5. If a gas’s temperature increases, what happens to the pressure and volume? a ...
... _____ 4. Benzene, C6H6, boils at 80.1˚C and has a density of 0.877 g/cm3. Determine the quantity of heat that is required to vaporize a 45.6 mL sample of benzene at 35.0˚C. a. 3140 J b. 4370 J c. 15800 J d. 18900 J _____ 5. If a gas’s temperature increases, what happens to the pressure and volume? a ...
Exam 1
... A. absorb mainly red light and therefore allow red light to pass through the solution. B. absorb mainly red light and therefore allow blue light to pass through the solution. C. absorb mainly blue light and therefore allow red light to pass through the solution. D. absorb mainly blue light and there ...
... A. absorb mainly red light and therefore allow red light to pass through the solution. B. absorb mainly red light and therefore allow blue light to pass through the solution. C. absorb mainly blue light and therefore allow red light to pass through the solution. D. absorb mainly blue light and there ...
BERKELEY HEIGHTS PUBLIC SCHOOLS
... 16. Compare and contrast regions of the electromagnetic spectrum, relating them to the wave probability model of the atom and orbital theory. (5.3 D/1; 5.6 A/8; 5.7 A/4) 17. Interpret Mendeleev’s first and Moseley’s modern periodic tables descriptions of metals, nonmetals, and metalloids in terms of ...
... 16. Compare and contrast regions of the electromagnetic spectrum, relating them to the wave probability model of the atom and orbital theory. (5.3 D/1; 5.6 A/8; 5.7 A/4) 17. Interpret Mendeleev’s first and Moseley’s modern periodic tables descriptions of metals, nonmetals, and metalloids in terms of ...
Chapter 6
... A student carries out an experiment to standardize a sodium hydroxide solution. To do this, the student weighs out 1.3009 g sample of potassium hydrogen phthalate (KHC8H4O4 or KHP–molar mass 204.22 g/mol). The student dissolves the KHP in distilled water, adds phenolphthalein as an indicator, and ti ...
... A student carries out an experiment to standardize a sodium hydroxide solution. To do this, the student weighs out 1.3009 g sample of potassium hydrogen phthalate (KHC8H4O4 or KHP–molar mass 204.22 g/mol). The student dissolves the KHP in distilled water, adds phenolphthalein as an indicator, and ti ...
CH 17 Study Guide with answer Key
... reactants and products, changing the volume of the reaction vessel causes no (11) ________________________ in the equilibrium. Changing the temperature of a reaction at equilibrium alters both the equilibrium (12) ________________________ and the equilibrium position. When a reaction is (13) _______ ...
... reactants and products, changing the volume of the reaction vessel causes no (11) ________________________ in the equilibrium. Changing the temperature of a reaction at equilibrium alters both the equilibrium (12) ________________________ and the equilibrium position. When a reaction is (13) _______ ...
Chemistry Final Test 1999-2000 - Nashoba Valley Technical High
... 17) Which of the following represents a pair of isotopes? A. 1H1+ and 11Na1+ B. 54Cr and 54Mn C. 31P3- and 80Br1D. 32S and 35S 18) The three main types of nuclear radiation are alpha, beta, and gamma. Which of the following lists these types of radiation from lest dangerous to most dangerous? A. alp ...
... 17) Which of the following represents a pair of isotopes? A. 1H1+ and 11Na1+ B. 54Cr and 54Mn C. 31P3- and 80Br1D. 32S and 35S 18) The three main types of nuclear radiation are alpha, beta, and gamma. Which of the following lists these types of radiation from lest dangerous to most dangerous? A. alp ...
1 - Study Hungary
... 20 protons, 19 neutrons, 19 electrons 19 protons, 20 neutrons, 18 electrons 39 protons, 19 neutrons, 38 electrons 20 protons, 19 neutrons, 20 electrons 40 protons, 20 neutrons, 19 electrons ...
... 20 protons, 19 neutrons, 19 electrons 19 protons, 20 neutrons, 18 electrons 39 protons, 19 neutrons, 38 electrons 20 protons, 19 neutrons, 20 electrons 40 protons, 20 neutrons, 19 electrons ...
Chemical Equilibrium
... Changing the volume of a reactant container changes the concentration of gaseous reactants and therefore their partial pressures Equilibrium position will therefore move The value of Kc or Kp does NOT change Changing pressure by adding more of an inert gas has no effect of the equilibrium position - ...
... Changing the volume of a reactant container changes the concentration of gaseous reactants and therefore their partial pressures Equilibrium position will therefore move The value of Kc or Kp does NOT change Changing pressure by adding more of an inert gas has no effect of the equilibrium position - ...
File
... • To balance an equation means to change the numbers of each molecule involved, so that the same number of atoms of each element appear on the reactants side and on the products side. • Chemical equations balance on an atomic level, not molecular. • You cannot change the formula of a substance, i.e. ...
... • To balance an equation means to change the numbers of each molecule involved, so that the same number of atoms of each element appear on the reactants side and on the products side. • Chemical equations balance on an atomic level, not molecular. • You cannot change the formula of a substance, i.e. ...
Chapter 4
... 1. Divide cations from anions in each reactant: BaCI2 (aq) + Na2SO4 (aq) Ba2+(aq) + 2Cl-(aq) + 2Na+(aq)+ SO4 2-(aq) 2. Match cation from one salt with the anion from the other salt” Ba2+(aq) + Cl-(aq) + Na+(aq)+ SO4 2-(aq) NaCl+ BaSO4 Note: Always keep the metal on the left in all salts! 3. Balanc ...
... 1. Divide cations from anions in each reactant: BaCI2 (aq) + Na2SO4 (aq) Ba2+(aq) + 2Cl-(aq) + 2Na+(aq)+ SO4 2-(aq) 2. Match cation from one salt with the anion from the other salt” Ba2+(aq) + Cl-(aq) + Na+(aq)+ SO4 2-(aq) NaCl+ BaSO4 Note: Always keep the metal on the left in all salts! 3. Balanc ...
Objectives - hartman
... • Calculate the amount in moles of a reactant or a product from the amount in moles of a different reactant or product. • Calculate the mass of a reactant or a product from the amount in moles of a different reactant or product. ...
... • Calculate the amount in moles of a reactant or a product from the amount in moles of a different reactant or product. • Calculate the mass of a reactant or a product from the amount in moles of a different reactant or product. ...
Unit 2:
... after each of the following disturbances is applied to the original mixture. For each case, assume that all other variables remain constant except for the given disturbance. Explain each answer with a short statement. (a) Additional H2(g) is added to the equilibrium mixture at constant volume. (b) T ...
... after each of the following disturbances is applied to the original mixture. For each case, assume that all other variables remain constant except for the given disturbance. Explain each answer with a short statement. (a) Additional H2(g) is added to the equilibrium mixture at constant volume. (b) T ...
Chemical Reaction
... If you place a thermometer in a beaker filled with a solution undergoing an endothermic reaction, the temp will go down. • Ex. Baking soda and vinegar © OUP: To be used solely in purchaser’s school or college ...
... If you place a thermometer in a beaker filled with a solution undergoing an endothermic reaction, the temp will go down. • Ex. Baking soda and vinegar © OUP: To be used solely in purchaser’s school or college ...
chemistry_chapter_3
... If the numbers are both whole numbers, these will be the subscripts of the elements in the formula If the whole numbers are identical, substitute the number 1 Example: C2H2 and C8H8 have an empirical formula of CH If either or both numbers are not whole numbers, numbers in the ratio must be mu ...
... If the numbers are both whole numbers, these will be the subscripts of the elements in the formula If the whole numbers are identical, substitute the number 1 Example: C2H2 and C8H8 have an empirical formula of CH If either or both numbers are not whole numbers, numbers in the ratio must be mu ...
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.