Chapter 18 Review Reaction Rates and Equilibrium Chapter
Chapter 18 Review “Reaction Rates and Equilibrium”
Chapter 18 Review n Energy that is available to do work is called ____. n ____ is defined as the number of atoms, ions, or molecules that react in a given time to form products. n What is the name of the minimum energy that colliding particles must have in order to react?
Chapter 18 Review n A substance that interferes with a catalyst is a(n) ____. n What is the arrangement of atoms at the peak of an energy barrier? n At equilibrium, what is the rate of production of reactants compared with the rate of production of products?
Chapter 18 Review n What is the equilibrium constant expression for the following reaction: C(s) + O 2(g) ↔ CO 2(g) n Which of the following is true about the combustion of carbon: a) the reaction is spontaneous, or b) entropy decreases? n The rate of a chemical reaction normally ____ as reactant concentration increases.
Chapter 18 Review n Why does a higher concentration make a reaction faster? n The amount of disorder in a system is measured by its ____. n Entropy measures ____ n What units represent a reaction rate? n For a complex reaction, the reaction progress curve has several ____.
Chapter 18 Review n What happens to a reaction at equilibrium when more reactant is added to the system? n Which reaction results in the greatest increase in entropy: a) A → B, or b) A → 2 B n If a reaction has an equilibrium constant (Keq) just greater than 1, how do we interpret that information?
Chapter 18 Review n. A catalyst works by ____. n If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction? n Which variable is NOT required to calculate the Gibbs free-energy change for a chemical reaction: a) change in enthalpy, or b) temperature in o. C?
Chapter 18 Review n What is the effect of adding more water to the following equilibrium reaction: CO 2 + H 2 O ↔ H 2 CO 3 n In an endothermic reaction at equilibrium, what is the effect of raising the temperature? n The energy that is available to do work in a reaction is called ____.
Chapter 18 Review n What is the numerical value (+ or -) of Gibbs free-energy change for a spontaneous reaction? n At what stage of a reaction do atoms have the highest energy? n Which of the following systems has the highest entropy: a) 10 m. L of water at 50 o. C, or b) 10 m. L of water at 100 o. C?
Chapter 18 Review n What happens to a catalyst in a reaction? n Write the rate law for the following reaction: A + 2 B → C + D n An elementary reaction converts reactants to products in ____. n Activation energy is ____. n Is the melting of ice at a temperature above 0 o. C: a) endothermic, or b) exothermic?
Chapter 18 Review n Consider the reaction: N 2(g) + 3 H 2(g) ↔ 2 NH 3(g) What is the effect of decreasing the volume on the contained gases? n Spontaneous reactions always ____ free energy. n Why does a higher temperature cause a reaction to go faster?
Chapter 18 Review n What 2 factors determine whether or not a reaction is spontaneous? n If a reaction is reversible, what are the relative amounts of reactant and product at the end of the reaction? n What physical state of nitrogen has the highest entropy? n What is another name for the catalysts in your body?
Chapter 18 Review n What is the order of the following reaction: A + 2 B → C + D n Why does a catalyst cause a reaction to proceed faster? n In an equilibrium reaction with a Keq of 1 x 108, the ____ are favored. n Which of the following explains why melting of ice is spontaneous at room temperature and pressure: a) it is accompanied by an increase in entropy, or b) it is accompanied by an increase in energy?
Chapter 18 Review n The Keq of a reaction is 4 x 10 -7. At equilibrium, the ____ are favored. n Another name for the activated complex is ____. n Which change would shift the following reaction to the right: 4 HCl(g) + O 2(g) ↔ 2 Cl 2(g) + 2 H 2 O(g) a) decrease of pressure, or b) increase of pressure?
Chapter 18 Review n In which of these systems is the entropy decreasing: a) salt dissolving in water, or b) a liquid cooling? n Given: 2 NCl. O(g) ↔ 2 NO(g) + Cl 2(g) An analysis of the equilibrium mixture in a 1 L flask is: NCl. O = 1. 6 mol; NO = 6. 4 mol; Cl 2 = 0. 49 mol. Calculate the value of Keq.
Chapter 18 Review n In a two-step reaction mechanism, how many elementary reactions occur?
Chapter 18 Review n. A mixture of hydrogen and iodine are in equilibrium with hydrogen iodide, as shown in the equation: H 2 + I 2 ↔ 2 HI Calculate the concentration of HI when the Keq is 1 x 105, the equilibrium concentration of H 2 is 0. 04 M, and the equilibrium concentration of I 2 is 0. 009 M.
Chapter 18 Review
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