Final Exam Review Guide
... 2. Concentrated and dilute are relative terms for expressing the concentration of a solution qualitatively. 3. Solutes and solvents are the two components of a solution. Thermochemistry Unit: 1. The collision theory explains that gas-phase chemical reactions occur when molecules collide with suffici ...
... 2. Concentrated and dilute are relative terms for expressing the concentration of a solution qualitatively. 3. Solutes and solvents are the two components of a solution. Thermochemistry Unit: 1. The collision theory explains that gas-phase chemical reactions occur when molecules collide with suffici ...
chm3400testfin
... c) The heat capacity of solid phosphorus in the vicinity of absolute zero is given by the expression Cp,m = aT3 + bT4 ...
... c) The heat capacity of solid phosphorus in the vicinity of absolute zero is given by the expression Cp,m = aT3 + bT4 ...
Exam #2
... (a) Electron affinities decrease going down the group (from smaller to larger elements). (b) Ionization energies decrease going down the group (from smaller to larger elements). (c) Chemical reactivity decreases going down the group (from smaller to larger elements). (d) The second ionization energy ...
... (a) Electron affinities decrease going down the group (from smaller to larger elements). (b) Ionization energies decrease going down the group (from smaller to larger elements). (c) Chemical reactivity decreases going down the group (from smaller to larger elements). (d) The second ionization energy ...
+ H 2
... • Consider the following reactions of three unknown metals X, Y and Z. 2XNO3(aq) + Y(s) → 2X(s) + Y(NO3)2(aq) Y(NO3)2(aq) + Z(s) → No reaction 2XNO3(aq) + Z(s) → 2X(s) + Z(NO3)2(aq) What is the order of increasing reactivity of the metals (least reactive first)? X < Z < Y ...
... • Consider the following reactions of three unknown metals X, Y and Z. 2XNO3(aq) + Y(s) → 2X(s) + Y(NO3)2(aq) Y(NO3)2(aq) + Z(s) → No reaction 2XNO3(aq) + Z(s) → 2X(s) + Z(NO3)2(aq) What is the order of increasing reactivity of the metals (least reactive first)? X < Z < Y ...
Types of Chemical Reactions
... Types of decomposition reactions – Decomposition of Binary Compounds – Decomposition of Metal Carbonates – Decomposition of Metal Hydroxides – Decomposition of Metal Chlorates – Decomposition of Acids ...
... Types of decomposition reactions – Decomposition of Binary Compounds – Decomposition of Metal Carbonates – Decomposition of Metal Hydroxides – Decomposition of Metal Chlorates – Decomposition of Acids ...
inorganic-chemistry-gp-i-alkali-metals
... Lithium shows different properties due to its extremely small size and lesser metallic character so as it shows significance similarity to Mg and other group II , which is a general trend and can be assumed to be a general perception. Due to high reactivity they do not occur in free state in nature ...
... Lithium shows different properties due to its extremely small size and lesser metallic character so as it shows significance similarity to Mg and other group II , which is a general trend and can be assumed to be a general perception. Due to high reactivity they do not occur in free state in nature ...
Ch_5_OpenStax_Chemistry edited
... 1. The sign of ΔH indicates whether the reaction is endothermic or exothermic at constant pressure. 2. The coefficients of the thermochemical equation represent the number of moles of reactants and products and can be used to derive useful conversion ...
... 1. The sign of ΔH indicates whether the reaction is endothermic or exothermic at constant pressure. 2. The coefficients of the thermochemical equation represent the number of moles of reactants and products and can be used to derive useful conversion ...
Chemical Reactions Chapter 11
... SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions. SC2.a. Identify and balance the following types of chemical equations: Synthesis, Decomposition, Single Replacement, Double Replacement, and Combustion SC2.b. ...
... SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions. SC2.a. Identify and balance the following types of chemical equations: Synthesis, Decomposition, Single Replacement, Double Replacement, and Combustion SC2.b. ...
Chemistry 1A Final Exam December 12, 2001 Page 1 of 16 (Closed
... 2.) (40 pts) Consider the dissociation of molecular chlorine (Cl2) to atomic chlorine (Cl): Cl2 → 2 Cl a) (15 pts) The bond enthalpy of the Cl-Cl bond is 242 kJ / mol. What is the maximum wavelength (λ, in nm) of light required to break the bond? For 1 mole of bonds: E = hν(6.02 x 1023) = 242 kJ / m ...
... 2.) (40 pts) Consider the dissociation of molecular chlorine (Cl2) to atomic chlorine (Cl): Cl2 → 2 Cl a) (15 pts) The bond enthalpy of the Cl-Cl bond is 242 kJ / mol. What is the maximum wavelength (λ, in nm) of light required to break the bond? For 1 mole of bonds: E = hν(6.02 x 1023) = 242 kJ / m ...
A.P. Chemistry
... M = mol/L Volume in liters (be sure to convert mL L) (p. 145-147) Problem: What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H2SO4 solution? ...
... M = mol/L Volume in liters (be sure to convert mL L) (p. 145-147) Problem: What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H2SO4 solution? ...
Unit 3, Lesson 07: Calculating ∆H using Standard Enthalpies of
... ∆H for a chemical reaction can be measured or calculated using: 1. Calorimetry data for chemical reactions • at constant pressure: – ∆H = Q = m · c · ∆T 2. Hess’s Law when you know ∆H values for other chemical reactions that can be added to give you your target chemical reaction 3. Standard Molar En ...
... ∆H for a chemical reaction can be measured or calculated using: 1. Calorimetry data for chemical reactions • at constant pressure: – ∆H = Q = m · c · ∆T 2. Hess’s Law when you know ∆H values for other chemical reactions that can be added to give you your target chemical reaction 3. Standard Molar En ...
AP® Chemistry 2009 Free-Response Questions - AP Central
... NO CALCULATORS MAY BE USED FOR PART B. Answer Question 4 below. The Section II score weighting for this question is 10 percent. 4. For each of the following three reactions, write a balanced equation in part (i) and answer the question in part (ii). In part (i), coefficients should be in terms of lo ...
... NO CALCULATORS MAY BE USED FOR PART B. Answer Question 4 below. The Section II score weighting for this question is 10 percent. 4. For each of the following three reactions, write a balanced equation in part (i) and answer the question in part (ii). In part (i), coefficients should be in terms of lo ...
Enthalpy - ChemGod.com
... Ea = Activation Energy The tale of a reaction is not limited strictly to the identity and energetics of the products and reactants, there is a path (reaction coordinate) that must get followed. The “hump” represents a hurdle that must be overcome to go from reactants to products. ...
... Ea = Activation Energy The tale of a reaction is not limited strictly to the identity and energetics of the products and reactants, there is a path (reaction coordinate) that must get followed. The “hump” represents a hurdle that must be overcome to go from reactants to products. ...
GCSE_C2_Revision_+_Exam_Questions
... The total number of protons and neutrons in an atom is called its mass number. Atoms of the same element can have different numbers of neutrons; these atoms are called isotopes of that element. The relative atomic mass of an element (Ar) compares the mass of atoms of the element with the 12C isotope ...
... The total number of protons and neutrons in an atom is called its mass number. Atoms of the same element can have different numbers of neutrons; these atoms are called isotopes of that element. The relative atomic mass of an element (Ar) compares the mass of atoms of the element with the 12C isotope ...
Balancing Equations Notes
... Chemical Equation: a way to represent chemical reactions on paper. Animation http://www.chemistry.ohio-state.edu/betha/nealChemBal/ ...
... Chemical Equation: a way to represent chemical reactions on paper. Animation http://www.chemistry.ohio-state.edu/betha/nealChemBal/ ...
Transition state theory
Transition state theory (TST) explains the reaction rates of elementary chemical reactions. The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and activated transition state complexes.TST is used primarily to understand qualitatively how chemical reactions take place. TST has been less successful in its original goal of calculating absolute reaction rate constants because the calculation of absolute reaction rates requires precise knowledge of potential energy surfaces, but it has been successful in calculating the standard enthalpy of activation (Δ‡Hɵ), the standard entropy of activation (Δ‡Sɵ), and the standard Gibbs energy of activation (Δ‡Gɵ) for a particular reaction if its rate constant has been experimentally determined. (The ‡ notation refers to the value of interest at the transition state.)This theory was developed simultaneously in 1935 by Henry Eyring, then at Princeton University, and by Meredith Gwynne Evans and Michael Polanyi of the University of Manchester. TST is also referred to as ""activated-complex theory,"" ""absolute-rate theory,"" and ""theory of absolute reaction rates.""Before the development of TST, the Arrhenius rate law was widely used to determine energies for the reaction barrier. The Arrhenius equation derives from empirical observations and ignores any mechanistic considerations, such as whether one or more reactive intermediates are involved in the conversion of a reactant to a product. Therefore, further development was necessary to understand the two parameters associated with this law, the pre-exponential factor (A) and the activation energy (Ea). TST, which led to the Eyring equation, successfully addresses these two issues; however, 46 years elapsed between the publication of the Arrhenius rate law, in 1889, and the Eyring equation derived from TST, in 1935. During that period, many scientists and researchers contributed significantly to the development of the theory.